This document contains multiple choice and short answer questions testing knowledge of basic chemistry concepts. It includes questions about the mole concept, stoichiometry, gas laws, solutions, and atomic structure. Specifically, students are asked to calculate molarity, molality, and mass percent; identify limiting reagents; and determine which laws are being followed in given chemical reactions.
Course Name (Legal Political and Ethical Dimensions of Business)MG.docxvanesaburnand
Course Name (Legal Political and Ethical Dimensions of Business)MGMT520
Week 2: Assignment Instructions
In each week the learning assignment is designed to demonstrate your competence with the Terminal Course Objectives of the course. Prior to working on the assignment, you should read through the week’s chapters and lesson.
Clearly identify your work with your name, the date, the week number and the assignment name, and upload work to the Dropbox.
The questions are designed to probe the higher levels of thinking and learning such as analyzing, evaluating and creating, and so there often are no “correct” answers. Instead of focusing and who wins or loses the case, you should analyze, evaluate and create alternative solutions to the various issues presented while arguing and debating the connections between business, law, politics and ethics.
Terminal Course Objective: G
Case Study: International and World Trade Law - Counterfeiting
Write a 1-2 page reflective paper (double spaced) on the following questions while discussing the connections between business, law, politics and ethics.
One: There has been a movement in the last decade encouraging people to “buy American.” Discuss the legal and ethical issues related to boycotting goods from other countries. What are the practical business implications of such a move?
Two: The World Trade Organization, or WTO, is the largest and most influential of the trade organizations. China and other heavy counterfeiting nations are part of this group. What could WTO-participating nations do to address the problems of counterfeiting? What should they do?
Three: The United Nations Security Council, the main decision-making body at the UN, is comprised of five regular members: China, France, the Russian Federation, the United Kingdom and the United States. Ten more members are elected from the General Assembly. Given the make-up of the committee, what type of action might the UN take with regard to the counterfeiting issue?
Submit your assignment to the Dropbox.
· 10165 - CHEM - 131 - Section 001 - Spring 2016 - General Chemistry Lec II
Top of Form
Question 1
Correct
Mark 3.00 out of 3.00
Flag question
Question text
All of the following are clues that a chemical reaction has taken place except
The reactant is smaller.
a.A flame occurs.
b.A color change occurs.
c. A solid forms.
Question 2
Question text
Balance the following equation in standard form and determine the sum of the coefficients.
a.6
b.4
c.3
d.14
e.7
Question 3
Question text
Balance this equation using the smallest possible integers, S + HNO3 → H2SO4 + NO2 + H2O. What is the coefficient of water.
Select one:
a.2
b.6
c.8
d. 1
e.
Question 4
Question text
When the following equation is balanced using the smallest possible integers, what is the coefficent of oxygen gas?
C7H16(g) + O2(g) → CO2(g) + H2O(g)
a.5
b.11
c.2
d.14
e.8
Question 5
Question text
True or false? The equation N2 + 3H2 → 2NH3 means that 1 g of N.
Course Name (Legal Political and Ethical Dimensions of Business)MG.docxvanesaburnand
Course Name (Legal Political and Ethical Dimensions of Business)MGMT520
Week 2: Assignment Instructions
In each week the learning assignment is designed to demonstrate your competence with the Terminal Course Objectives of the course. Prior to working on the assignment, you should read through the week’s chapters and lesson.
Clearly identify your work with your name, the date, the week number and the assignment name, and upload work to the Dropbox.
The questions are designed to probe the higher levels of thinking and learning such as analyzing, evaluating and creating, and so there often are no “correct” answers. Instead of focusing and who wins or loses the case, you should analyze, evaluate and create alternative solutions to the various issues presented while arguing and debating the connections between business, law, politics and ethics.
Terminal Course Objective: G
Case Study: International and World Trade Law - Counterfeiting
Write a 1-2 page reflective paper (double spaced) on the following questions while discussing the connections between business, law, politics and ethics.
One: There has been a movement in the last decade encouraging people to “buy American.” Discuss the legal and ethical issues related to boycotting goods from other countries. What are the practical business implications of such a move?
Two: The World Trade Organization, or WTO, is the largest and most influential of the trade organizations. China and other heavy counterfeiting nations are part of this group. What could WTO-participating nations do to address the problems of counterfeiting? What should they do?
Three: The United Nations Security Council, the main decision-making body at the UN, is comprised of five regular members: China, France, the Russian Federation, the United Kingdom and the United States. Ten more members are elected from the General Assembly. Given the make-up of the committee, what type of action might the UN take with regard to the counterfeiting issue?
Submit your assignment to the Dropbox.
· 10165 - CHEM - 131 - Section 001 - Spring 2016 - General Chemistry Lec II
Top of Form
Question 1
Correct
Mark 3.00 out of 3.00
Flag question
Question text
All of the following are clues that a chemical reaction has taken place except
The reactant is smaller.
a.A flame occurs.
b.A color change occurs.
c. A solid forms.
Question 2
Question text
Balance the following equation in standard form and determine the sum of the coefficients.
a.6
b.4
c.3
d.14
e.7
Question 3
Question text
Balance this equation using the smallest possible integers, S + HNO3 → H2SO4 + NO2 + H2O. What is the coefficient of water.
Select one:
a.2
b.6
c.8
d. 1
e.
Question 4
Question text
When the following equation is balanced using the smallest possible integers, what is the coefficent of oxygen gas?
C7H16(g) + O2(g) → CO2(g) + H2O(g)
a.5
b.11
c.2
d.14
e.8
Question 5
Question text
True or false? The equation N2 + 3H2 → 2NH3 means that 1 g of N.
Chapter 4 Problems1. Which of these compounds is a strong elec.docxketurahhazelhurst
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of ...
Chapter 4 Problems1. Which of these compounds is a strong elec.docxrobertad6
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of.
Chem 1010 Name__________________________________
Unit 4-5 Test
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) When the following equation is balanced, the coefficient of Al is __________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 4
B) 1
C) 3
D) 5
E) 2
2) When the following equation is balanced, the coefficient of NaOH is __________.
H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)
A) 1
B) 4
C) 2
D) 0
E) 3
3) When the following equation is balanced, the coefficient of O2 is __________.
C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)
A) 5
B) 3
C) 4
D) 2
E) 1
4) When the following equation is balanced, the coefficient of C3H8O3 is __________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 2
B) 5
C) 7
D) 1
E) 3
1
5) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium
phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq)
B) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)
C) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)
E) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)
6) When the reaction shown is correctly balanced, the coefficients are:
C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)
A) 1, 3.5, 6, 7
B) 2, 16.5, 12, 7
C) 2, 15, 12, 6
D) 1, 9.5, 6, 7
E) 1, 6, 6, 7
7) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.
A) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
B) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)
C) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
D) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
E) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
8) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) H+ and OH-
B) Mg2+ and H+
C) H+ and Cl-
D) OH- only
E) Mg2+ and Cl-
9) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is
________.
A) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
B) Ag+ (aq) + I- (aq) → AgI (s)
C) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)
D) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
E) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
10) A neutralization reaction between an acid and a metal hydroxide produces ________.
A) oxygen gas
B) sodium hydroxide
C) ammonia
D) water and a salt
E) hydrogen gas
2
11) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
B) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)
C) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) H+ (aq) + OH- (aq) → H2O (l)
12) Which of the following is an oxidation-reduction reaction?
A) Pb(C2H3O2)2(aq) + 2 NaCl(.
ENG 107 Commentary 1HW for Tu, April 19th – Commentary .docxSALU18
ENG 107 Commentary 1
HW for Tu, April 19th – Commentary Paper Proposal
1. Choose the trend about which you will be writing your commentary.
2. Go to Google / images; type “you trend name stats” and find a recent chart/graph that represents this trend. Note, you graph has to come with an article.
3. Examine the chart/graph; try to read it and understand what it says.
4. Write a 1p. long Paper Proposal.
1. Insert the graph/chart
2. Write 1 paragraph in which you introduce and explain this graph to us.
i. The graph on Figure 1 represents the trend of …..(name the trend). The graph was made ion …. by…. This graph shows …. . We can also see that ….. Another obvious tendency shown in this graph is that …. . Finally, it is evident that ….
ii. The information presented in this trend made me think that ….
3. What is the significance of this trend? Why did you choose to write your commentary about this trend?
4. Read the article that comes with the trend. Write a short annotation to this article:
· You introduce your source:
I found an article (a website) on the Internet written (created) by ………..and publishedin (a newspaper) /on (a website) in… (date).
· Briefly summarize the main idea of the article:
From this article I learned that… . I also discovered that …. … . It was new to me that … Likewise I found out that... It turns out that… Moreover, I learned that… So-So’s (name of the author) article made me wonder… / think of … (Author’s Last Name / “Title of the Article”).
· Quote one or 2 sentences that you found especially interesting.
I found it especially interesting that So-So (author) says/ believes/ suggests/… that “……..your quotation goes here” (Author’s Last Name / “Title of the Article”).
· Your commentary / response to the article:
These words made me think that….
1
Practice Problems -- Set #4 (chap 9 and 10)
1. MgCl2 is a(an)
(A). acid
(B). base
(C). salt
(D). covalent compound
2. Which one of the compounds is insoluble in water (hint: solubility rules)
(A). BaSO4
(B). NaCl
(C). KI
(D). HCl
(E). All of the above are soluble in water.
3. Identify a strong base.
(A). HNO3
(B). KCl
(C). NH4OH
(D). NaOH
(E). Na2SO4
4. Acid-base reaction is a neutralization reaction. If 12.50 mL of 1.20 M NaOH solution is used to
neutralize 45.25 mL of HNO3 solution, calculate the concentration of the original HNO3
solution.
(A). 0.231 M
(B). 0.995 M
(C). 0.887 M
(D). 0.331 M
(E). 9.90 M
5. Acid-base reaction is a neutralization reaction. If 12.50 mL of 1.20 M NaOH solution is used to
neutralize 45.25 mL of H2SO4 solution, calculate the concentration of the original H2SO4
solution.
2NaOH + H2SO4 Na2SO4 + 2H2O (balanced?)
(A). 0.231 M
(B). 0.995 M
(C). 0.887 M
(D). 0.166 M
(E). 0.331 M
6. Oxidation-reduction (redox) reactions involve electrons. If an element in ground state loses two
electrons during the redox reaction, this process ...
Chapter 4 Problems1. Which of these compounds is a strong elec.docxketurahhazelhurst
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of ...
Chapter 4 Problems1. Which of these compounds is a strong elec.docxrobertad6
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of.
Chem 1010 Name__________________________________
Unit 4-5 Test
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) When the following equation is balanced, the coefficient of Al is __________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 4
B) 1
C) 3
D) 5
E) 2
2) When the following equation is balanced, the coefficient of NaOH is __________.
H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)
A) 1
B) 4
C) 2
D) 0
E) 3
3) When the following equation is balanced, the coefficient of O2 is __________.
C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)
A) 5
B) 3
C) 4
D) 2
E) 1
4) When the following equation is balanced, the coefficient of C3H8O3 is __________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 2
B) 5
C) 7
D) 1
E) 3
1
5) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium
phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq)
B) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)
C) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)
E) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)
6) When the reaction shown is correctly balanced, the coefficients are:
C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)
A) 1, 3.5, 6, 7
B) 2, 16.5, 12, 7
C) 2, 15, 12, 6
D) 1, 9.5, 6, 7
E) 1, 6, 6, 7
7) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.
A) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
B) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)
C) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
D) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
E) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
8) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) H+ and OH-
B) Mg2+ and H+
C) H+ and Cl-
D) OH- only
E) Mg2+ and Cl-
9) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is
________.
A) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
B) Ag+ (aq) + I- (aq) → AgI (s)
C) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)
D) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
E) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
10) A neutralization reaction between an acid and a metal hydroxide produces ________.
A) oxygen gas
B) sodium hydroxide
C) ammonia
D) water and a salt
E) hydrogen gas
2
11) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
B) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)
C) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) H+ (aq) + OH- (aq) → H2O (l)
12) Which of the following is an oxidation-reduction reaction?
A) Pb(C2H3O2)2(aq) + 2 NaCl(.
ENG 107 Commentary 1HW for Tu, April 19th – Commentary .docxSALU18
ENG 107 Commentary 1
HW for Tu, April 19th – Commentary Paper Proposal
1. Choose the trend about which you will be writing your commentary.
2. Go to Google / images; type “you trend name stats” and find a recent chart/graph that represents this trend. Note, you graph has to come with an article.
3. Examine the chart/graph; try to read it and understand what it says.
4. Write a 1p. long Paper Proposal.
1. Insert the graph/chart
2. Write 1 paragraph in which you introduce and explain this graph to us.
i. The graph on Figure 1 represents the trend of …..(name the trend). The graph was made ion …. by…. This graph shows …. . We can also see that ….. Another obvious tendency shown in this graph is that …. . Finally, it is evident that ….
ii. The information presented in this trend made me think that ….
3. What is the significance of this trend? Why did you choose to write your commentary about this trend?
4. Read the article that comes with the trend. Write a short annotation to this article:
· You introduce your source:
I found an article (a website) on the Internet written (created) by ………..and publishedin (a newspaper) /on (a website) in… (date).
· Briefly summarize the main idea of the article:
From this article I learned that… . I also discovered that …. … . It was new to me that … Likewise I found out that... It turns out that… Moreover, I learned that… So-So’s (name of the author) article made me wonder… / think of … (Author’s Last Name / “Title of the Article”).
· Quote one or 2 sentences that you found especially interesting.
I found it especially interesting that So-So (author) says/ believes/ suggests/… that “……..your quotation goes here” (Author’s Last Name / “Title of the Article”).
· Your commentary / response to the article:
These words made me think that….
1
Practice Problems -- Set #4 (chap 9 and 10)
1. MgCl2 is a(an)
(A). acid
(B). base
(C). salt
(D). covalent compound
2. Which one of the compounds is insoluble in water (hint: solubility rules)
(A). BaSO4
(B). NaCl
(C). KI
(D). HCl
(E). All of the above are soluble in water.
3. Identify a strong base.
(A). HNO3
(B). KCl
(C). NH4OH
(D). NaOH
(E). Na2SO4
4. Acid-base reaction is a neutralization reaction. If 12.50 mL of 1.20 M NaOH solution is used to
neutralize 45.25 mL of HNO3 solution, calculate the concentration of the original HNO3
solution.
(A). 0.231 M
(B). 0.995 M
(C). 0.887 M
(D). 0.331 M
(E). 9.90 M
5. Acid-base reaction is a neutralization reaction. If 12.50 mL of 1.20 M NaOH solution is used to
neutralize 45.25 mL of H2SO4 solution, calculate the concentration of the original H2SO4
solution.
2NaOH + H2SO4 Na2SO4 + 2H2O (balanced?)
(A). 0.231 M
(B). 0.995 M
(C). 0.887 M
(D). 0.166 M
(E). 0.331 M
6. Oxidation-reduction (redox) reactions involve electrons. If an element in ground state loses two
electrons during the redox reaction, this process ...
We understand the unique challenges pickleball players face and are committed to helping you stay healthy and active. In this presentation, we’ll explore the three most common pickleball injuries and provide strategies for prevention and treatment.
Struggling with intense fears that disrupt your life? At Renew Life Hypnosis, we offer specialized hypnosis to overcome fear. Phobias are exaggerated fears, often stemming from past traumas or learned behaviors. Hypnotherapy addresses these deep-seated fears by accessing the subconscious mind, helping you change your reactions to phobic triggers. Our expert therapists guide you into a state of deep relaxation, allowing you to transform your responses and reduce anxiety. Experience increased confidence and freedom from phobias with our personalized approach. Ready to live a fear-free life? Visit us at Renew Life Hypnosis..
QA Paediatric dentistry department, Hospital Melaka 2020Azreen Aj
QA study - To improve the 6th monthly recall rate post-comprehensive dental treatment under general anaesthesia in paediatric dentistry department, Hospital Melaka
R3 Stem Cells and Kidney Repair A New Horizon in Nephrology.pptxR3 Stem Cell
R3 Stem Cells and Kidney Repair: A New Horizon in Nephrology" explores groundbreaking advancements in the use of R3 stem cells for kidney disease treatment. This insightful piece delves into the potential of these cells to regenerate damaged kidney tissue, offering new hope for patients and reshaping the future of nephrology.
Global launch of the Healthy Ageing and Prevention Index 2nd wave – alongside...ILC- UK
The Healthy Ageing and Prevention Index is an online tool created by ILC that ranks countries on six metrics including, life span, health span, work span, income, environmental performance, and happiness. The Index helps us understand how well countries have adapted to longevity and inform decision makers on what must be done to maximise the economic benefits that comes with living well for longer.
Alongside the 77th World Health Assembly in Geneva on 28 May 2024, we launched the second version of our Index, allowing us to track progress and give new insights into what needs to be done to keep populations healthier for longer.
The speakers included:
Professor Orazio Schillaci, Minister of Health, Italy
Dr Hans Groth, Chairman of the Board, World Demographic & Ageing Forum
Professor Ilona Kickbusch, Founder and Chair, Global Health Centre, Geneva Graduate Institute and co-chair, World Health Summit Council
Dr Natasha Azzopardi Muscat, Director, Country Health Policies and Systems Division, World Health Organisation EURO
Dr Marta Lomazzi, Executive Manager, World Federation of Public Health Associations
Dr Shyam Bishen, Head, Centre for Health and Healthcare and Member of the Executive Committee, World Economic Forum
Dr Karin Tegmark Wisell, Director General, Public Health Agency of Sweden
Defecation
Normal defecation begins with movement in the left colon, moving stool toward the anus. When stool reaches the rectum, the distention causes relaxation of the internal sphincter and an awareness of the need to defecate. At the time of defecation, the external sphincter relaxes, and abdominal muscles contract, increasing intrarectal pressure and forcing the stool out
The Valsalva maneuver exerts pressure to expel faeces through a voluntary contraction of the abdominal muscles while maintaining forced expiration against a closed airway. Patients with cardiovascular disease, glaucoma, increased intracranial pressure, or a new surgical wound are at greater risk for cardiac dysrhythmias and elevated blood pressure with the Valsalva maneuver and need to avoid straining to pass the stool.
Normal defecation is painless, resulting in passage of soft, formed stool
CONSTIPATION
Constipation is a symptom, not a disease. Improper diet, reduced fluid intake, lack of exercise, and certain medications can cause constipation. For example, patients receiving opiates for pain after surgery often require a stool softener or laxative to prevent constipation. The signs of constipation include infrequent bowel movements (less than every 3 days), difficulty passing stools, excessive straining, inability to defecate at will, and hard feaces
IMPACTION
Fecal impaction results from unrelieved constipation. It is a collection of hardened feces wedged in the rectum that a person cannot expel. In cases of severe impaction the mass extends up into the sigmoid colon.
DIARRHEA
Diarrhea is an increase in the number of stools and the passage of liquid, unformed feces. It is associated with disorders affecting digestion, absorption, and secretion in the GI tract. Intestinal contents pass through the small and large intestine too quickly to allow for the usual absorption of fluid and nutrients. Irritation within the colon results in increased mucus secretion. As a result, feces become watery, and the patient is unable to control the urge to defecate. Normally an anal bag is safe and effective in long-term treatment of patients with fecal incontinence at home, in hospice, or in the hospital. Fecal incontinence is expensive and a potentially dangerous condition in terms of contamination and risk of skin ulceration
HEMORRHOIDS
Hemorrhoids are dilated, engorged veins in the lining of the rectum. They are either external or internal.
FLATULENCE
As gas accumulates in the lumen of the intestines, the bowel wall stretches and distends (flatulence). It is a common cause of abdominal fullness, pain, and cramping. Normally intestinal gas escapes through the mouth (belching) or the anus (passing of flatus)
FECAL INCONTINENCE
Fecal incontinence is the inability to control passage of feces and gas from the anus. Incontinence harms a patient’s body image
PREPARATION AND GIVING OF LAXATIVESACCORDING TO POTTER AND PERRY,
An enema is the instillation of a solution into the rectum and sig
Telehealth Psychology Building Trust with Clients.pptxThe Harvest Clinic
Telehealth psychology is a digital approach that offers psychological services and mental health care to clients remotely, using technologies like video conferencing, phone calls, text messaging, and mobile apps for communication.
CRISPR-Cas9, a revolutionary gene-editing tool, holds immense potential to reshape medicine, agriculture, and our understanding of life. But like any powerful tool, it comes with ethical considerations.
Unveiling CRISPR: This naturally occurring bacterial defense system (crRNA & Cas9 protein) fights viruses. Scientists repurposed it for precise gene editing (correction, deletion, insertion) by targeting specific DNA sequences.
The Promise: CRISPR offers exciting possibilities:
Gene Therapy: Correcting genetic diseases like cystic fibrosis.
Agriculture: Engineering crops resistant to pests and harsh environments.
Research: Studying gene function to unlock new knowledge.
The Peril: Ethical concerns demand attention:
Off-target Effects: Unintended DNA edits can have unforeseen consequences.
Eugenics: Misusing CRISPR for designer babies raises social and ethical questions.
Equity: High costs could limit access to this potentially life-saving technology.
The Path Forward: Responsible development is crucial:
International Collaboration: Clear guidelines are needed for research and human trials.
Public Education: Open discussions ensure informed decisions about CRISPR.
Prioritize Safety and Ethics: Safety and ethical principles must be paramount.
CRISPR offers a powerful tool for a better future, but responsible development and addressing ethical concerns are essential. By prioritizing safety, fostering open dialogue, and ensuring equitable access, we can harness CRISPR's power for the benefit of all. (2998 characters)
Navigating the Health Insurance Market_ Understanding Trends and Options.pdfEnterprise Wired
From navigating policy options to staying informed about industry trends, this comprehensive guide explores everything you need to know about the health insurance market.
CHAPTER 1 SEMESTER V - ROLE OF PEADIATRIC NURSE.pdfSachin Sharma
Pediatric nurses play a vital role in the health and well-being of children. Their responsibilities are wide-ranging, and their objectives can be categorized into several key areas:
1. Direct Patient Care:
Objective: Provide comprehensive and compassionate care to infants, children, and adolescents in various healthcare settings (hospitals, clinics, etc.).
This includes tasks like:
Monitoring vital signs and physical condition.
Administering medications and treatments.
Performing procedures as directed by doctors.
Assisting with daily living activities (bathing, feeding).
Providing emotional support and pain management.
2. Health Promotion and Education:
Objective: Promote healthy behaviors and educate children, families, and communities about preventive healthcare.
This includes tasks like:
Administering vaccinations.
Providing education on nutrition, hygiene, and development.
Offering breastfeeding and childbirth support.
Counseling families on safety and injury prevention.
3. Collaboration and Advocacy:
Objective: Collaborate effectively with doctors, social workers, therapists, and other healthcare professionals to ensure coordinated care for children.
Objective: Advocate for the rights and best interests of their patients, especially when children cannot speak for themselves.
This includes tasks like:
Communicating effectively with healthcare teams.
Identifying and addressing potential risks to child welfare.
Educating families about their child's condition and treatment options.
4. Professional Development and Research:
Objective: Stay up-to-date on the latest advancements in pediatric healthcare through continuing education and research.
Objective: Contribute to improving the quality of care for children by participating in research initiatives.
This includes tasks like:
Attending workshops and conferences on pediatric nursing.
Participating in clinical trials related to child health.
Implementing evidence-based practices into their daily routines.
By fulfilling these objectives, pediatric nurses play a crucial role in ensuring the optimal health and well-being of children throughout all stages of their development.
CHAPTER 1 SEMESTER V - ROLE OF PEADIATRIC NURSE.pdf
keep501 (1).pdf
1. 1. Two students performed the same experiment separately and each one of
them recorded two readings of mass which are given below. Correct reading
of mass is 3.0 g. On the basis of given data, mark the correct option out of the
following statements.
Student Readings
(i) (ii)
A 3.01 2.99
B 3.05 2.95
(i) Results of both the students are neither accurate nor precise.
(ii) Results of student A are both precise and accurate.
(iii) Results of student B are neither precise nor accurate.
(iv) Results of student B are both precise and accurate.
2. A measured temperature on Fahrenheit scale is 200 °F. What will this reading
be on Celsius scale?
(i) 40 °C
(ii) 94 °C
(iii) 93.3 °C
(iv) 30 °C
3. What will be the molarity of a solution, which contains 5.85 g of NaCl(s) per
500 mL?
(i) 4 mol L
–1
(ii) 20 mol L
–1
I. Multiple Choice Questions (Type-I)
16-04-2018
2. 2
Exemplar Problems, Chemistry
(iii) 0.2 mol L
–1
(iv) 2 mol L
–1
4. If 500 mL of a 5M solution is diluted to 1500 mL, what will be the molarity of
the solution obtained?
(i) 1.5 M
(ii) 1.66 M
(iii) 0.017 M
(iv) 1.59 M
5. The number of atoms present in one mole of an element is equal to Avogadro
number. Which of the following element contains the greatest number of
atoms?
(i) 4g He
(ii) 46g Na
(iii) 0.40g Ca
(iv) 12g He
6. If the concentration of glucose (C6
H12
O6
) in blood is 0.9 g L
–1
, what will be the
molarity of glucose in blood?
(i) 5 M
(ii) 50 M
(iii) 0.005 M
(iv) 0.5 M
7. What will be the molality of the solution containing 18.25 g of HCl gas in
500 g of water?
(i) 0.1 m
(ii) 1 M
(iii) 0.5 m
(iv) 1 m
8. One mole of any substance contains 6.022 × 1023
atoms/molecules. Number
of molecules of H2
SO4
present in 100 mL of 0.02M H2
SO4
solution is ______.
(i) 12.044 × 10
20
molecules
(ii) 6.022 × 10
23
molecules
(iii) 1 × 10
23
molecules
(iv) 12.044 × 10
23
molecules
9. What is the mass percent of carbon in carbon dioxide?
(i) 0.034%
(ii) 27.27%
16-04-2018
3. 3 Some Basic Concepts of Chemistry
(iii) 3.4%
(iv) 28.7%
10. The empirical formula and molecular mass of a compound are CH2
O and
180 g respectively. What will be the molecular formula of the compound?
(i) C9
H18
O9
(ii) CH2
O
(iii) C6
H12
O6
(iv) C2
H4
O2
11. If the density of a solution is 3.12 g mL
–1
, the mass of 1.5 mL solution in
significant figures is _______.
(i) 4.7g
(ii) 4680 × 10–3
g
(iii) 4.680g
(iv) 46.80g
12. Which of the following statements about a compound is incorrect?
(i) A molecule of a compound has atoms of different elements.
(ii) A compound cannot be separated into its constituent elements by
physical methods of separation.
(iii) A compound retains the physical properties of its constituent elements.
(iv) The ratio of atoms of different elements in a compound is fixed.
13. Which of the following statements is correct about the reaction given below:
4Fe(s) + 3O2
(g) → 2Fe2
O3
(g)
(i) Total mass of iron and oxygen in reactants = total mass of iron and
oxygen in product therefore it follows law of conservation of mass.
(ii) Total mass of reactants = total mass of product; therefore, law of multiple
proportions is followed.
(iii) Amount of Fe2
O3
can be increased by taking any one of the reactants
(iron or oxygen) in excess.
(iv) Amount of Fe2
O3
produced will decrease if the amount of any one of the
reactants (iron or oxygen) is taken in excess.
14. Which of the following reactions is not correct according to the law of
conservation of mass.
(i) 2Mg(s) + O2
(g) → 2MgO(s)
(ii) C3
H8
(g) + O2
(g) → CO2
(g) + H2
O(g)
(iii) P4
(s) + 5O2
(g) → P4
O10
(s)
(iv) CH4
(g) + 2O2
(g) → CO2
(g) + 2H2
O (g)
16-04-2018
4. 4
Exemplar Problems, Chemistry
15. Which of the following statements indicates that law of multiple proportion is
being followed.
(i) Sample of carbon dioxide taken from any source will always have carbon
and oxygen in the ratio 1:2.
(ii) Carbon forms two oxides namely CO2
and CO, where masses of oxygen
which combine with fixed mass of carbon are in the simple ratio 2:1.
(iii) When magnesium burns in oxygen, the amount of magnesium taken
for the reaction is equal to the amount of magnesium in magnesium
oxide formed.
(iv) At constant temperature and pressure 200 mL of hydrogen will combine
with 100 mL oxygen to produce 200 mL of water vapour.
II. Multiple Choice Questions (Type-II)
In the following questions two or more options may be correct.
16. One mole of oxygen gas at STP is equal to _______.
(i) 6.022 × 1023
molecules of oxygen
(ii) 6.022 × 1023
atoms of oxygen
(iii) 16 g of oxygen
(iv) 32 g of oxygen
17. Sulphuric acid reacts with sodium hydroxide as follows :
H2
SO4
+ 2NaOH → Na2
SO4
+ 2H2
O
When 1L of 0.1M sulphuric acid solution is allowed to react with 1L of 0.1M
sodium hydroxide solution, the amount of sodium sulphate formed and its
molarity in the solution obtained is
(i) 0.1 mol L
–1
(ii) 7.10 g
(iii) 0.025 mol L
–1
(iv) 3.55 g
18. Which of the following pairs have the same number of atoms?
(i) 16 g of O2
(g) and 4 g of H2
(g)
(ii) 16 g of O2
and 44 g of CO2
(iii) 28 g of N2
and 32 g of O2
(iv) 12 g of C(s) and 23 g of Na(s)
19. Which of the following solutions have the same concentration?
(i) 20 g of NaOH in 200 mL of solution
(ii) 0.5 mol of KCl in 200 mL of solution
16-04-2018
5. 5 Some Basic Concepts of Chemistry
(iii) 40 g of NaOH in 100 mL of solution
(iv) 20 g of KOH in 200 mL of solution
20. 16 g of oxygen has same number of molecules as in
(i) 16 g of CO
(ii) 28 g of N2
(iii) 14 g of N2
(iv) 1.0 g of H2
21. Which of the following terms are unitless?
(i) Molality
(ii) Molarity
(iii) Mole fraction
(iv) Mass percent
22. One of the statements of Dalton’s atomic theory is given below:
“Compounds are formed when atoms of different elements combine in a fixed
ratio”
Which of the following laws is not related to this statement?
(i) Law of conservation of mass
(ii) Law of definite proportions
(iii) Law of multiple proportions
(iv) Avogadro law
III. Short Answer Type
23. What will be the mass of one atom of C-12 in grams?
24. How many significant figures should be present in the answer of the following
calculations?
2.5 1.25 3.5
2.01
× ×
25. What is the symbol for SI unit of mole? How is the mole defined?
26. What is the difference between molality and molarity?
27. Calculate the mass percent of calcium, phosphorus and oxygen in calcium
phosphate Ca3
(PO4
)2
.
28. 45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous
oxide was formed. The reaction is given below:
2N2
(g) + O2
(g) → 2N2
O(g)
Which law is being obeyed in this experiment? Write the statement of the law?
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6. 6
Exemplar Problems, Chemistry
29. If two elements can combine to form more than one compound, the masses of
one element that combine with a fixed mass of the other element, are in whole
number ratio.
(a) Is this statement true?
(b) If yes, according to which law?
(c) Give one example related to this law.
30. Calculate the average atomic mass of hydrogen using the following data :
Isotope % Natural abundance Molar mass
1
H 99.985 1
2
H 0.015 2
31. Hydrogen gas is prepared in the laboratory by reacting dilute HCl with
granulated zinc. Following reaction takes place.
Zn + 2HCl → ZnCl2
+ H2
Calculate the volume of hydrogen gas liberated at STP when 32.65 g of zinc
reacts with HCl. 1 mol of a gas occupies 22.7 L volume at STP; atomic mass of
Zn = 65.3 u.
32. The density of 3 molal solution of NaOH is 1.110 g mL
–1
. Calculate the molarity
of the solution.
33. Volume of a solution changes with change in temperature, then, will the molality
of the solution be affected by temperature? Give reason for your answer.
34. If 4 g of NaOH dissolves in 36 g of H2
O, calculate the mole fraction of each
component in the solution. Also, determine the molarity of solution (specific
gravity of solution is 1g mL
–1
).
35. The reactant which is entirely consumed in reaction is known as limiting reagent.
In the reaction 2A + 4B → 3C + 4D, when 5 moles of A react with 6 moles of B,
then
(i) which is the limiting reagent?
(ii) calculate the amount of C formed?
IV. Matching Type
36. Match the following:
(i) 88 g of CO2
(a) 0.25 mol
(ii) 6.022 ×1023
molecules of H2
O (b) 2 mol
(iii) 5.6 litres of O2
at STP (c) 1 mol
(iv) 96 g of O2
(d) 6.022 × 1023
molecules
(v) 1 mol of any gas (e) 3 mol
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7. 7 Some Basic Concepts of Chemistry
37. Match the following physical quantities with units
Physical quantity Unit
(i) Molarity (a) g mL
–1
(ii) Mole fraction (b) mol
(iii) Mole (c) Pascal
(iv) Molality (d) Unitless
(v) Pressure (e) mol L
–1
(vi) Luminous intensity (f) Candela
(vii) Density (g) mol kg–1
(viii) Mass (h) Nm–1
(i) kg
V. Assertion and Reason Type
In the following questions a statement of Assertion (A) followed by a
statement of Reason (R) is given. Choose the correct option out of the
choices given below each question.
38. Assertion (A) : The empirical mass of ethene is half of its molecular mass.
Reason (R) : The empirical formula represents the simplest whole number
ratio of various atoms present in a compound.
(i) Both A and R are true and R is the correct explanation of A.
(ii) A is true but R is false.
(iii) A is false but R is true.
(iv) Both A and R are false.
39. Assertion (A) : One atomic mass unit is defined as one twelfth of the mass of
one carbon-12 atom.
Reason (R) : Carbon-12 isotope is the most abundunt isotope of carbon
and has been chosen as standard.
(i) Both A and R are true and R is the correct explanation of A.
(ii) Both A and R are true but R is not the correct explanation of A.
(iii) A is true but R is false.
(iv) Both A and R are false.
40. Assertion (A) : Significant figures for 0.200 is 3 where as for 200 it is 1.
Reason (R) : Zero at the end or right of a number are significant provided
they are not on the right side of the decimal point.
(i) Both A and R are true and R is correct explanation of A.
(ii) Both A and R are true but R is not a correct explanation of A.
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8. 8
Exemplar Problems, Chemistry
(iii) A is true but R is false.
(iv) Both A and R are false.
41. Assertion (A) : Combustion of 16 g of methane gives 18 g of water.
Reason (R) : In the combustion of methane, water is one of the products.
(i) Both A and R are true but R is not the correct explanation of A.
(ii) A is true but R is false.
(iii) A is false but R is true.
(iv) Both A and R are false.
VI. Long Answer Type
42. A vessel contains 1.6 g of dioxygen at STP (273.15K, 1 atm pressure). The
gas is now transferred to another vessel at constant temperature, where
pressure becomes half of the original pressure. Calculate
(i) volume of the new vessel.
(ii) number of molecules of dioxygen.
43. Calcium carbonate reacts with aqueous HCl to give CaCl2
and CO2
according
to the reaction given below:
CaCO3
(s) + 2HCl (aq) → CaCl2
(aq) + CO2
(g) + H2
O(l)
What mass of CaCl2
will be formed when 250 mL of 0.76 M HCl reacts with
1000 g of CaCO3
? Name the limiting reagent. Calculate the number of moles
of CaCl2
formed in the reaction.
44. Define the law of multiple proportions. Explain it with two examples. How
does this law point to the existance of atoms?
45. A box contains some identical red coloured balls, labelled as A, each weighing
2 grams. Another box contains identical blue coloured balls, labelled as B,
each weighing 5 grams. Consider the combinations AB, AB2
, A2
B and A2
B3
and show that law of multiple proportions is applicable.
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9. 9 Some Basic Concepts of Chemistry
ANSWERS
I. Multiple Choice Questions (Type-I)
1. (ii) 2. (iii) 3. (iii) 4. (ii) 5. (iv) 6. (iii)
7. (iv) 8. (i) 9. (ii) 10. (iii) 11. (i) 12. (iii)
13. (i) 14. (ii) 15. (ii)
II. Multiple Choice Questions (Type-II)
16. (i), (iv) 17. (ii), (iii) 18. (iii), (iv)
19. (i), (ii) 20. (iii), (iv) 21. (iii), (iv)
22. (i), (iv)
III. Short Answer Type
23. 1.992648 × 10–23
g ≈ 1.99 × 10–23
g
24. 2
25. Symbol for SI Unit of mole is mol.
One mole is defined as the amount of a substance that contains as many
particles or entities as there are atoms in exactly 12 g (0.012 kg) of the 12
C
isotope.
26. Molality is the number of moles of solute present in one kilogram of solvent
but molarity is the number of moles of solute dissolved in one litre of
solution.
Molality is independent of temperature whereas molarity depends on
temperature.
27. Mass percent of calcium = ×
3 4 2
3 × (atomic mass of calcium)
100
molecular mass of Ca (PO )
120 u
= ×100 = 38.71%
310 u
Mass percent of phosphorus = ×
3 4 2
2 × (atomic mass of phosphorus)
100
molecular mass of Ca (PO )
2 × 31 u
= ×100
310 u
= 20%
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10. 10
Exemplar Problems, Chemistry
Mass percent of oxygen
×
= ×
3 4 2
8 (Atomic mass of oxygen)
100
molecular mass of Ca (PO )
×
8 16 u
= ×100
310 u
= 41.29%
28. According to Gay Lussac’s law of gaseous volumes, gases combine or are
produced in a chemical reaction in a simple ratio by volume, provided
that all gases are at the same temperature and pressure.
29. (a) Yes
(b) According to the law of multiple proportions
(c) H2
+ O2
→ H2
O
2 g 16 g 18 g
(c) H2
+ O2
→ H2
O2
2 g 32 g 34 g
Here masses of oxygen, (i.e., 16 g in H2
O and 32 g in H2
O2
) which combine
with fixed mass of hydrogen (2 g) are in the simple ratio i.e., 16 : 32 or 1 : 2
30. Average Atomic Mass =
1
2 2
{(Natural abundance of H × molar mass) +
(Natural abundance of H × molar mass of H)}
100
× + ×
=
99.985 1 0.015 2
100
+
=
99.985 0.030
100
=
100.015
100
= 1.00015 u
31. From the equation, 63.5 g of zinc liberates 22.7 litre of hydrogen. So
32.65 g of zinc will liberate
2
22.7 L H
32.65 g Zn ×
65.3 g Zn
=
22.7
L = 11.35 L
2
32. 3 molal solution of NaOH means that 3 mols of NaOH are dissolved in
1000 g of solvent.
∴ Mass of Solution = Mass of Solvent + Mass of Solute
= 1000 g + (3 × 40 g) = 1120 g
Volume of Solution = =
1120
mL 1009.00
1.110
mL
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11. 11 Some Basic Concepts of Chemistry
(Since density of solution = 1.110g mL
–1
)
Since 1009 mL solution contains 3 mols of NaOH
∴ Molarity
Number of moles of solute
=
Volume of solution in litre
= ×
3 mol
1000
1009.00
= 2.97 M
33. No, Molality of solution does not change with temperature since mass
remains unaffected with temperature.
34. Mass of NaOH = 4 g
Number of moles of =
4 g
NaOH = 0.1 mol
40 g
Mass of H2
O = 36 g
Number of moles of =
2
36 g
H O = 2 mol
18 g
Mole fraction of water
2
Number of moles of H O
=
No. of moles of water + No. of moles of NaOH
= =
2 2
= 0.95
2 + 0.1 2.1
Mole fraction of NaOH =
Number of moles of NaOH
No. of moles of NaOH + No. of moles of water
= =
0.1 0.1
= 0.047
2 + 0.1 2.1
Mass of solution = mass of water + mass of NaOH = 36 g + 4 g = 40 g
Volume of solution = 40 × 1 = 40 mL
(Since specific gravity of solution is = 1 g mL
–1
)
Molarity of solution
Number of moles of solute
=
Volume of solution in litre
0.1 mol NaOH
= = 2.5 M
0.04 L
35. 2A + 4B → 3C + 4D
According to the above equation, 2 mols of ‘A’ require 4 mols of ‘B’ for the
reaction.
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12. 12
Exemplar Problems, Chemistry
Hence, for 5 mols of ‘A’, the moles of ‘B’ required =
4 mol of B
5 mol of A ×
2 mol of A
= 10 mol B
But we have only 6 mols of ‘B’, hence, ‘B’ is the limiting reagent. So amount
of ‘C’ formed is determined by amount of ‘B’.
Since 4 mols of ‘B’ give 3 mols of ‘C’. Hence 6 mols of ‘B’ will give
3 mol of C
6 mol of B ×
4 mol of B
= 4.5 mol of C
IV. Matching Type
36. (i) → (b) (ii) → (c) (iii) → (a) (iv) → (e)
(v) → (d)
37. (i) → (e) (ii) → (d) (iii) → (b) (iv) → (g)
(v) → (c), (h) (vi) → (f) (vii) → (a) (viii) → (i)
V. Assertion and Reason Type
38. (i) 39. (ii) 40. (iii) 41. (iii)
VI. Long Answer Type
42. (i) p1
=1 atm, T1
=273 K, V1
=?
32 g of oxygen occupies 22.4 L of volume at STP*
Hence,1.6 g of oxygen will occupy,
22.4 L
1.6 g oxygen ×
32 g oxygen
= 1.12 L
V1
=1.12 L
p
p 1
2
1
= = = 0.5 atm.
2 2
V2
=?
According to Boyle’s law :
p1
V1
= p2
V2
p V
V
p
1 1
2
2
×
= 1 atm. × 1.12 L
=
0.5 atm.
= 2.24 L
* Old STP conditions 273.15 K, 1 atm, volume occupied by 1 mol of gas = 22.4 L.
New STP conditions 273.15 K, 1 bar, volume occupied by a gas = 22.7 L.
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13. 13 Some Basic Concepts of Chemistry
(ii) Number of molecules of oxygen in the vessel =
× ×
23
6.022 10 1.6
32
= 3.011 × 1022
43. Number of moles of HCl = 250 mL ×
0.76 M
1000
= 0.19 mol
Mass of CaCO3
= 1000 g
Number of moles of CaCO3
= =
1000 g
10
100 g
mol
According to given equation 1 mol of CaCO3
(s) requires 2 mol of HCl (aq).
Hence, for the reaction of 10 mol of CaCO3
(s) number of moles of HCl
required would be:
3
3
2 mol HCl (aq)
10 mol CaCO ×
1 mol CaCO (s) = 20 mol HCl (aq)
But we have only 0.19 mol HCl (aq), hence, HCl (aq) is limiting reagent.
So amount of CaCl2
formed will depend on the amount of HCl available.
Since, 2 mol HCl (aq) forms 1 mol of CaCl2
, therefore, 0.19 mol of HCl (aq)
would give:
0.19 mol HCl (aq) ×
2
1 mol CaCl (aq)
2 mol HCl (aq)
= 0.095 mol
or 0.095 × molar mass of CaCl2
= 0.095 × 111 = 10.54 g
45. (Hint : Show that the masses of B which combine with the fixed mass of
A in different combinations are related to each other by simple whole
numbers).
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