In 1500 Words use the provided sources in each parts to answer the following question in APA 7th Ed style · Part 1 of 2 (refer to Week 3 Readings in the Lessons for Week 3) · Evaluate: 1. What are different kinds of insider threats to our US cyber security? 2. What mitigation efforts can help address this concern? 3. Does corruption and cyber infrastructure have anything in common? What are they and what can be done to help address this concern? · Conclude with a research or policy question for further research. Sources for the Part 1: Insider Threat from the Department of Homeland Security https://www.dhs.gov/science-and-technology/cybersecurity-insider-threat CISA: Insider Threat Mitigation https://www.cisa.gov/insider-threat-mitigation · Part 2 of 2 (refer to Week 4 Readings in the Lessons for Week 4) 1) How does social media assist emergency management. Give examples.       2) How does social media hinder emergency management. Give examples.       3) How can emergency management officials help assist with providing relevant and detailed information about public health concerns? · Conclude with a research or policy question. Sources for the Part 2: Innovative uses in Social Media  https://www.dhs.gov/sites/default/files/publications/Social-Media-EM_0913-508_0.pdf IS-0042: Social Media in Emergency Management  https://emilms.fema.gov/is_0042/curriculum/1.html Experiment 11. Percent Yield of a Chemical Reaction LEARNING OBJECTIVES: 1. Students will be able to predict the amount of product produced from a double displacement reaction and determine the percent yield of a chemical reaction. 2. Students will be able to identify the limiting and excess reactants. BACKGROUND. Stoichiometry is the mole to mole relationships between the reactants and the products of a chemical reaction. Stoichiometric calculations are about the amounts of substances that react (reactants) and form (products) in chemical reactions. Chemical reactions are represented by equations which are balanced using the smallest wholenumber coefficients. A balanced chemical equation helps the chemist to calculate the amounts of product formed in a chemical reaction. This is the theoretical yield of the reaction. In other words, it is the maximum amount of product that can be obtained in a particular reaction from a known quantity of reactants. This may not be always the case and the amount of product obtained in a chemical reaction is usually less than the theoretical amount. The amount of product obtained in a chemical reaction performed in the laboratory is called the actual yield. The percent yield of a reaction is then given by the following expression: Actual Yield Percent yield =× 100 Theoritical Yield In this experiment, you will react Na2CO3 and CaCl2. You will prepare calcium carbonate, CaCO3, from the reaction of aqueous solution of sodium carbonate, Na2CO3, with the aqueous solution of calcium chloride, CaCl2. From the amounts of the reactants, you will ...

1. In 1500 Words use the provided sources in each parts to answer
the following question in APA 7th Ed style
· Part 1 of 2 (refer to Week 3 Readings in the Lessons for Week
3)
· Evaluate:
1. What are different kinds of insider threats to our US cyber
security?
2. What mitigation efforts can help address this concern?
3. Does corruption and cyber infrastructure have anything in
common? What are they and what can be done to help address
this concern?
· Conclude with a research or policy question for further
research.
Sources for the Part 1:
Insider Threat from the Department of Homeland
Security https://www.dhs.gov/science-and-
technology/cybersecurity-insider-threat
CISA: Insider Threat Mitigation https://www.cisa.gov/insider-
threat-mitigation
· Part 2 of 2 (refer to Week 4 Readings in the Lessons for Week
4)
1) How does social media assist emergency management. Give
examples.
2) How does social media hinder emergency management.
Give examples.
3) How can emergency management officials help assist
with providing relevant and detailed information about public
health concerns?
· Conclude with a research or policy question.
Sources for the Part 2:

2. Innovative uses in Social Media
https://www.dhs.gov/sites/default/files/publications/Social -
Media-EM_0913-508_0.pdf
IS-0042: Social Media in Emergency Management
https://emilms.fema.gov/is_0042/curriculum/1.html
Experiment 11.
Percent Yield of a Chemical Reaction
LEARNING OBJECTIVES:
1. Students will be able to predict the amount of product
produced from a double displacement reaction and determine
the percent yield of a chemical reaction.
2. Students will be able to identify the limiting and excess
reactants.
BACKGROUND.
Stoichiometry is the mole to mole relationships between the
reactants and the products of a chemical reaction.
Stoichiometric calculations are about the amounts of substances
that react (reactants) and form (products) in chemical reactions.
Chemical reactions are represented by equations which are
balanced using the smallest wholenumber coefficients. A
balanced chemical equation helps the chemist to calculate the
amounts of product formed in a chemical reaction. This is the
theoretical yield of the reaction. In other words, it is the
maximum amount of product that can be obtained in a particular
reaction from a known quantity of reactants. This may not be
always the case and the amount of product obtained in a
chemical reaction is usually less than the theoretical amount.

3. The amount of product obtained in a chemical reaction
performed in the laboratory is called the actual yield. The
percent yield of a reaction is then given by the following
expression:
Actual Yield
Percent yield =× 100
Theoritical Yield
In this experiment, you will react Na2CO3 and CaCl2. You will
prepare calcium carbonate, CaCO3, from the reaction of
aqueous solution of sodium carbonate, Na2CO3, with the
aqueous solution of calcium chloride, CaCl2. From the amounts
of the reactants, you will determine which reactant is the
limiting reactant, and from this amount, will calculate the
theoretical yield of calcium carbonate produced. From the
actual amount of calcium carbonate obtained, you can then
calculate your percent yield of reaction.
The balanced equation for this chemical reaction is: CaCl2(aq)
+ Na2CO3(aq
The net ionic equation of the reaction is:
Ca2+(aq) + CO32-
(aq) and (s) mean aqueous and precipitate or solid, respectively.
SAFETY INSTRUCTIONS
1. Wear your eye goggles at all times.
2. All chemicals used in these experiments are generally
recognized as safe. But, you MUST wash your hands after you
finish the experiment.
3. If your instructor recommends you use vacuum filtration,
proceed with caution. The side arm of the Erlenmeyer can
break.
MATERIALS
Centigram balance, ring stand, O-ring, funnel, filter paper, clay

4. triangle, spatula, stirring rod, 50-mL graduated cylinder, two
150-mL beakers, watch glass, pencil, solid sodium carbonate,
0.50 M sodium carbonate solution.
PRE-LABORATORY WORKED EXAMPLE.
A student adds 30.0 mL of 0.10 M potassium chromate into a
beaker containing 100.0 mL 0.010 M silver nitrate solution. The
precipitate is filtered, washed and dried. The mass of the solid
product is 0.15 gram. Cr = 52; Ag = 108; O = 16; N = 14; K =
39.
Note: The molarity of a solution is the number of moles of
solute in 1.0 Liter of solution.
Note: The number of moles of solute is, mole = Molarity ×
Volume
a. Write the balanced equation representing the chemical
reaction.
3(aq)
b. Write the net ionic equation of the chemical reaction.
2Ag+(aq) + CrO42-
c. Determine the number of moles of each reactant.
nAgNO3 = M × V = 0.010 mol.L-1 × 0.100 L = 0.0010 mol
AgNO3 nK2CrO4
= M × V = 0.10 mol.L-1 × 0.030 L = 0.0030 mol K2CrO4
d. Identify the limiting reactant. Note: Lesser amount is the
limiting reactant.
1mol Ag CrO 332 g Ag CrO

5. 0.0010 mol AgNO3 × 2 4 × 2 4
2 mol AgNO3 1mol Ag2CrO4
= 0.166 g Ag2CrO4
1mol Ag CrO 332 g Ag CrO
0.0030 mol K2CrO4 × 2 4 × 2 4
= 0.996 g Ag2CrO4
1mol K CrO2 4 1mol Ag2CrO4
The limiting reactant is AgNO3.
e. Determine the theoretical yield of the reaction.
The theoretical yield of the reaction is 0.166 g.
f. Calculate the percent yield of the reaction.
Actual Yield 0.15
Percent yield =× 100 =× 100 = 88%
Theoritical Yield 0.17
PRE-LABORATORY QUESTION NAME:
A student weighs 1.00 gram of zinc powder and places it into a
beaker containing 25.00 mL of a 0.50
M CuCl2 solution. After the reaction is completed, the solid
(metallic copper) is recovered from the
bottom of the beaker, filtered, washed with hydrochloric acid
solution, and dried completely. The mass of the precipitate is
0.72 gram. Zn = 65, Cu = 63.5C; Cl = 35.5.
1. Write the equation representing the chemical reacti on.

6. 2. Determine the number of moles of zinc reactant present.
3. Determine the number of moles of CuCl2 reactant present
4. Calculate the theoretical yield of the reaction.
5. Calculate the percent yield of this reaction.
EXPERIMENTAL PROCEDURE
1. Using a pencil, write your name on the edges of the filter
paper, and place it on a watch glass.Weigh the filter paper and
the watch glass together.
2. Weigh an empty 150-mL beaker and record its mass.
3. Place about 1.00 gram of the powdered sodium carbonate,
Na2CO3, into the beaker, and weigh it again. Record the mass.

7. 4. Dissolve the solid using about 25 to 30 mL of deionized
water.
5. Using the 50-mL graduated cylinder, measure 50.0 mL of
0.50 M CaCl2 solution.
6. Add the CaCl2 solution into the beaker containing the
Na2CO3 solution. Observe the precipitation reaction. Mix the
mixture with a stirring rod.
7. Assemble the stand, O-ring, funnel, and filter paper
according to the figure described below. Filter the mixture.
8. Wash the residue twice with 5.0 mL of deionized water.
Rinse with isopropyl alcohol and dry in theoven for half an
hour.
9. Carefully remove the filter paper and precipitate and place it
on the watch glass.
10. Give the watch glass to your instructor.
11. Weigh the filter paper, dried residue, and watch glass.
Record the mass.
12. Calculate the percent yield of the reaction.
DATE:

8. DATA SHEET FOR EXPERIMENT 11.
NAME:
TRIAL 1
TRIAL 2
1. Mass of the filter paper and the watch glass:
g
g
2. Mass of the beaker:
g
g
3. Mass of the beaker + Na2CO3:
g
g
4. Mass of the Na2CO3: (line 3) – (line 2)
g
g
g
g
5. Mass of the dried residue, watch glass, and filter paper:

9. g
g
6. Mass of the CaCO3 (residue): Actual Yield: (line 5) – (line 1)
g
g
7. Theoretical yield# of CaCO3: (From stoichiometric
calculations)
%
%
8. Percent Yield of the reaction: [(line 6) / (line 7)] × 100
8. Average percent yield:
%
#Use the following stoichiometric calculations to determine the
theoretical yield.
106grams 1mol Na2CO3 1molCaCO3
grams CaCO3
1molCaCl2 1molCaCO3
grams CaCO3

10. POSTLAB QUESTIONS NAME:
1. A sample of 30.00 grams of potassium phosphate was added
to a solution containing 100.0 mL of 0.25 M calcium nitrate.
Calcium phosphate was precipitated according to the following
reaction.
2.25 grams of Calcium phosphate were recovered. Calculate the
theoretical yield and the percent yield.
2. A student adds 50.0 mL of 0.25 M K2SO4 solution to 25.0
mL 0.50 M BaCl2 solution. What is the mass of the precipitate
that can be recovered if the percent yield of the reaction is
75%? Ba = 137; Cl = 35.5; S = 32 O = 16; K = 39. Note: You
must write the balanced equation first.
3. A 4.00-gram sample of sodium chloride was added to a
beaker containing 40.0 mL 0.033 M
lead(II) nitrate solution. Lead(II) chloride was precipitated
according to the following reaction.

11. Calculate the mass of lead(II) chloride that can be recovered. Pb
= 207; Na = 23; Cl = 35.5; N = 14; O
= 16.
4. A student adds 50.0 mL of 0.25 M KCl solution to 25.0 mL
0.50 M AgNO3 solution. What is the mass of the precipitate that
can be recovered if the percent yield of the reaction is 90%? Ag
= 108; Cl
= 35.5; N = 14; O = 16; K = 39. Note: You must write the
balanced equation first.