This document discusses Universal Children's Day, which is observed annually on November 20. In 1954, the United Nations General Assembly recommended that countries introduce an annual event to encourage understanding between children worldwide and promote children's welfare. While countries could choose their own date, many opted to observe it on November 20th to respect this UN recommendation. Universal Children's Day aims to improve children's lives globally through international cooperation and understanding.
The Avogadro constant, represents the number of carbon-12 atoms in exactly 12 g of pure carbon-12. the value of Avogadro constant is 6.0221421 푥 10^23. How many atoms of K-40 (Radioactive isotope) are present in 225 mL of whole milk containing 1.65 mg K/mL?
The Avogadro constant, represents the number of carbon-12 atoms in exactly 12 g of pure carbon-12. the value of Avogadro constant is 6.0221421 푥 10^23. How many atoms of K-40 (Radioactive isotope) are present in 225 mL of whole milk containing 1.65 mg K/mL?
Description
This infographic presents the theories that have been formulated about the structure of the atom. Each theory is accompanied with a basic description and a comparison is sought between them.
Objectives
After the completion of this lesson, students will be able to:
- Understand the differences between the pre-quantum and quantum theories.
- Understand the experimental data that led to the progress of the theories.
- Describe the structural components of matter as well as their properties.
Activities
1. Democritus’ theory: Students have to think about how small matter can get, to understand the meaning of the word ‘atomos’ and to understand that this specific theory was impossible to prove.
2. Dalton’s theory: Students have to discuss the reason that Dalton is considered as the father of the atomic theory despite the fact that Democritus had the original idea.
3. Thomson’s theory: The teacher introduces the discovery of electrons and challenges students to consider the structure of plum pudding in order to explain the specific theory.
4. Rutherford’s model: The teacher asks students to enlarge the atom to the size of football court in order to understand that the nucleus will be the size of a ping-pong ball. The students watch the animated video of Rutherford’s model.
5. Bohr’s model: Students have to observe images of the last two models and discuss the similarities and differences. Students have to explore the structure of different atoms through the simulation link.
6. Quantum Mechanical model: The teacher asks students to observe specific images with different meanings in order to introduce the double nature of an electron. Students have to understand that electrons exist as ‘probability clouds.’
Erasmus+ Project: Educational Infographics For STEAM
https://steam-edu.eu
NOMENCLATURE OF BINARY POLY-ATOMIC COMPOUNDSGrinty Babu
Giving names to chemical compounds, formulae, common polyatomic atoms. introduction about binary compounds, ionic bonds. provided with examples of binary ionic compounds.
Description
This infographic presents the theories that have been formulated about the structure of the atom. Each theory is accompanied with a basic description and a comparison is sought between them.
Objectives
After the completion of this lesson, students will be able to:
- Understand the differences between the pre-quantum and quantum theories.
- Understand the experimental data that led to the progress of the theories.
- Describe the structural components of matter as well as their properties.
Activities
1. Democritus’ theory: Students have to think about how small matter can get, to understand the meaning of the word ‘atomos’ and to understand that this specific theory was impossible to prove.
2. Dalton’s theory: Students have to discuss the reason that Dalton is considered as the father of the atomic theory despite the fact that Democritus had the original idea.
3. Thomson’s theory: The teacher introduces the discovery of electrons and challenges students to consider the structure of plum pudding in order to explain the specific theory.
4. Rutherford’s model: The teacher asks students to enlarge the atom to the size of football court in order to understand that the nucleus will be the size of a ping-pong ball. The students watch the animated video of Rutherford’s model.
5. Bohr’s model: Students have to observe images of the last two models and discuss the similarities and differences. Students have to explore the structure of different atoms through the simulation link.
6. Quantum Mechanical model: The teacher asks students to observe specific images with different meanings in order to introduce the double nature of an electron. Students have to understand that electrons exist as ‘probability clouds.’
Erasmus+ Project: Educational Infographics For STEAM
https://steam-edu.eu
NOMENCLATURE OF BINARY POLY-ATOMIC COMPOUNDSGrinty Babu
Giving names to chemical compounds, formulae, common polyatomic atoms. introduction about binary compounds, ionic bonds. provided with examples of binary ionic compounds.
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.
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Personal development courses are widely available today, with each one promising life-changing outcomes. Tim Han’s Life Mastery Achievers (LMA) Course has drawn a lot of interest. In addition to offering my frank assessment of Success Insider’s LMA Course, this piece examines the course’s effects via a variety of Tim Han LMA course reviews and Success Insider comments.
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Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
for Anti-inflammatory, Antiulcer, Anticancer, Wound healing, Antidiabetic, Hepatoprotective, Cardio protective, Diuretics and
Antifertility, Toxicity studies as per OECD guidelines
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The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
Chapter 3 - Islamic Banking Products and Services.pptx
Stoichiometry Practice Problems
1. Name: ……………………………………
Grade: …………10………………
Subject: Chemistry
Date: ……………….
Chapter 15 : Stoichiometry Practice Problems
Be sure to balance all equations before you start calculating
Rally coach :
1) Lithium hydroxide reacts with hydrobromic acid to produce lithium bromide and water. If
you start with 10 grams of lithium hydroxide, how many grams of lithium bromide will be
produced? LiOH + HBr LiBr + H2O
2) Ethylene (C2H4 ) reacts with oxygen gas to produce carbon dioxide and water. If you start
with 45 grams of ethylene, how many grams of carbon dioxide will be produced?
C2H4 + 3 O2 2 CO2 + 2 H2O
3) Be + 2 HCl BeCl2 + H2
My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5 grams,
what was my percent yield?
2. 4) Given the equation: HCl + Na2SO4 NaCl + H2SO4
If you start with 20 grams of hydrochloric acid, how many grams of sulfuric acid will be
produced?
5) Given the following equation: LiOH + KCl LiCl + KOH
a. I began this reaction with 20 grams of lithium hydroxide. What is my theoretical
yield of lithium chloride?
b. I actually produced 6 grams of lithium chloride. What is my percent yield?
6) Given the following equation: C3H8 + O2 CO2 + H2O
a. If I start with 5 grams of C3H8, what is my theoretical yield of water?
b. I got a percent yield of 75%. How many grams of water did I make?
7) Given the reaction: NaCl + CaO CaCl2 + Na2O
What is my theoretical yield of sodium oxide if I start with 20 grams of calcium oxide?
3. 8) FeBr2 + 2 KCl FeCl2 + 2 KBr
a. What is my theoretical yield of iron (II) chloride if I start with 34 grams of iron (II)
bromide?
b. What is my percent yield of iron (II) chloride if my actual yield is 4 grams?
9) TiS + H2O H2S + TiO
What is my percent yield of titanium (II) oxide if I start with 20 grams of titanium (II)
sulfide and my actual yield of titanium (II) oxide is 22 grams?
10) U + 3 Br2 UBr6
What is my actual yield of uranium hexabromide if I start with 100 grams of uranium and
250 grams of bromine, and get a percent yield of 83% ?
11) Sulfur dioxide can be produced in the laboratory by the reaction of hydrochloric acid and a
sulfite salt such as sodium sulfite. (Na2SO3 + 2HCl → 2NaCl + SO2 + H2O) What mass
of SO2 can be made from 25.0 g or Na2SO3 and 22.0 g of HCl?
Name: grade: date:
4. Mole & Mass Conversions
1. What is the mass (in grams) of 1.00 moles of copper atoms?
1.00mol Cu x 63.5 g Cu = 63.5g Cu
1 mol Cu
2. How many moles are 4.00g of helium atoms?
4.00g He x 1 mol He = 1.00 mol He
4.00 g He
3. What is the mass of 3.56 moles of zinc?
3.56mol Zn x 65.4 g Zn = 233g Zn
1 mol Zn
4. What is the mass of 1.00 moles of water molecules?
1.00mol H2O x 18.0 g H2O = 18.0g H2O
1 mol H2O
5. How many moles are found in 7.95g of lithium chloride?
7.95g LiCl x 1 mol LiCl = 0.188 mol LiCl
42.4 g LiCl
6. What is the mass of 4.50mol of aluminum chloride?
4.50mol AlCl3 x 134 g AlCl3= 603g AlCl3
1 mol AlCl3
7. Convert 250g of calcium hydroxide into moles.
250g Ca(OH)2 x 1 mol Ca(OH)2 = 3.37 mol Ca(OH)2
74.1 g Ca(OH)2
8. You are given 365g of sugar (C6H12O6)
a) How many moles would you have?
365g C6H12O6 x 1 mol C6H12O6= 2.03 mol C6H12O6
5. Answer Key
1) LiOH + HBr LiBr + H2O
If you start with ten grams of lithium hydroxide, how many grams of lithium bromide will
be produced? 36.3 grams
2) C2H4 + 3 O2 2 CO2 + 2 H2O
If you start with 45 grams of ethylene (C2H4), how many grams of carbon dioxide will be
produced? 141.4 grams
3) 2 HCl + Na2SO4 2 NaCl + H2SO4
If you start with 20 grams of hydrochloric acid, how many grams of sulfuric acid will be
produced? 26.9 grams
4) Given the following equation: LiOH + KCl LiCl + KOH
a. I began this reaction with 20 grams of lithium hydroxide. What is my theoretical
yield of lithium chloride? 35.5 grams
b. I actually produced 6 grams of lithium chloride. What is my percent yield? 16.9%
5) Given the following equation: C3H8 + 5 O2 3 CO2 + 4 H2O
a. If I start with 5 grams of C3H8, what is my theoretical yield of water? 8.2 grams
b. I got a percent yield of 75%. How many grams of water did I make? 6.1 grams
6) Be + 2 HCl BeCl2 + H2
My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5
grams, what was my percent yield? 42.1 %
7) Given the reaction: 2 NaCl + CaO CaCl2 + Na2O
What is my theoretical yield of sodium oxide if I start with 20 grams of calcium oxide?
22.1 grams
8) FeBr2 + 2 KCl FeCl2 + 2 KBr
a. What is my theoretical yield of iron (II) chloride if I start with 34 grams of iron (II)
bromide? 20.0 grams of FeCl2
b. What is my percent yield of iron (II) chloride if my actual yield is 4 grams? 20 %
9) TiS + H2O H2S + TiO
What is my percent yield of titanium (II) oxide if I start with 20 grams of titanium (II)
sulfide and my actual yield of titanium (II) oxide is 22 grams? 137.5 % (theoretical yield is
16.0 grams—trick question; you should know that 100% is the highest yield possible)
10) U + 3 Br2 UBr6
What is my actual yield of uranium hexabromide if I start with 100 grams of uranium and
250 grams of bromine, and get a percent yield of 83% ? 250 grams UBr6
6. 11) Sulfur dioxide can be produced in the laboratory by the reaction of hydrochloric acid and a
sulfite salt such as sodium sulfite. (Na2SO3 + 2HCl → 2NaCl + SO2 + H2O) What mass of
SO2 can be made from 25.0 g or Na2SO3 and 22.0 g of HCl? 11.3 grams SO2
7. Universal Children's Day
On December 14, 1954, the United Nations General Assembly recommended
that all countries should introduce an annual event from 1956 known as
Universal Children's Day to encourage understanding between children all
over the world and promoting the welfare of children.
It was recommended that individual countries should choose an appropriate
date for this occasion.
Many of the countries respected this recommendation and the Universal
Children's Day has since been annually observed on November 20.