Module Five Assignment Name: Chemical Equations Instructions: Solve the following chemical equations

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Module Five Assignment

Name:

Chemical Equations

Instructions: Solve the following chemical equations.

1) For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts.

2) For the following reaction, calculate how many moles of each product are formed when 0.326 moles of PbS completely react. Assume there is an excess of oxygen.

3) For the following reaction, calculate how many moles of each product are formed when 4.05 g of water is used.

4) Determine the theoretical yield of P2O5, when 3.07 g of P reacts with 6.09 g of oxygen in the following chemical equation

5) Determine the percent yield of the following reaction when 2.30 g of P reacts with excess oxygen. The actual yield of this reaction is determined to by 4.89 g of P2O5.

Properties of Liquids and Solids

Instructions: Answer the following questions using the following information: ?Hfus=6.02 kJ/mol; ?Hvap= 40.7 kJ/mol; specific heat of water is 4.184 J/g??C; specific heat of ice is 2.06 J/g??C; specific heat of water vapor is 2.03 J/g??C.

1) How much heat is required to vaporize 30 g of water at 100?C?

 

 

 

 

 

2) How much heat is required to convert 29 g of ice at -4.0 ?C to water vapor at 105 ?C (report your answer to three significant figures)? Answer all five parts, showing your detailed calculations:

i) Heat to warm ice from -4.0 to 0 oC:

 

ii) Heat to convert ice to liquid:

 

 

iii) Heat to warm liquid to boiling:

 

iv) Heat to convert liquid to gas:

 

 

v) Heat to warm gas from 100 to 105 oC:

 

 

 

 

 

 

 

 

 

 

3. An ice cube at 0.00 ?C with a mass of 8.32 g is placed into 55 g of water, initially at 25 ?C. If no heat is lost to the surroundings, what is the final temperature of the entire water sample after all the ice is melted (report your answer to three significant figures)?

 

 

 

 

 

 

 

 

 

 

 

Mixtures and Solutions

Instructions: Use the following image to answer the following questions. Circle your answers and/or show your calculations.

1. A solution contains 40 g of NaCl per 100 g of water at 20?C. Is the solution unsaturated, saturated or supersaturated?

unsaturated, saturated or supersaturated?

 

 

2. A solution contains 50 g of KCl per 100 g of water at 90?C. Is the solution unsaturated, saturated or supersaturated?

unsaturated, saturated or supersaturated?

 

 

 

3. A solution contains 30 g of KNO3 per 100 g of water at 20?C. Is the solution unsaturated, saturated or supersaturated?

Solubility Graph [Online Image]. Retrieved November 12, 2018 from https://socratic.org/chemistry/solutions-and-their-behavior/solubility-graphs

 

 

unsaturated, saturated or supersaturated?

 

 

4. An 8 oz bottle of Dr. Pepper made with imperial cane sugar (C12H22O11) contains 27 g of sugar in 266.6 mL of water. What is the molarity of the solution with respect to cane sugar?

 

 

 

5. Calculate the mass of NaCl in a 55 mL sample of a 3.5 M saline solution.

 

 

 

6. What volume of water should be added to 4.6 g of KCl to make a 4 M solution?

 

 

 

Acid/Base: The Water Constant and pH

Instructions: Determine if each solution is acidic, basic, or neutral. Circle your answers.

Acidic Basic Neutral

 

1. [H3O+] = 1 x 10-10 M; [OH-] = 1 x 10-4 M

 

Acidic Basic Neutral

 

2. [H3O+] = 1 x 10-7 M; [OH-] = 1 x 10-7 M

 

Acidic Basic Neutral

 

3. [H3O+] = 1 x 10-1 M; [OH-] = 1 x 10-13 M

 

Acidic Basic Neutral

 

4. [H3O+] = 1 x 10-13 M; [OH-] = 1 x 10-1 M

 

Instructions: Calculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic.

[OH-] = Acidic Basic Neutral

 

5. [H3O+] = 2.6 x 10-3 M

 

[OH-] = Acidic Basic Neutral

 

6. [H3O+] = 3.6 x 10-8 M

 

[OH-] = Acidic Basic Neutral

 

7. [H3O+] = 3.6 x 10-2 M

 

[OH-] = Acidic Basic Neutral

 

8. [H3O+] = 4.3 x 10-3 M

 

Instructions: Calculate the [H3O+] of solutions a and b; calculate the [OH-] solutions c and d.

 

 

9.

 

 

Chemistry, Assignment 5, Fall 2020, Page 1 of 5

 

10. pH = 2.76

 

11. pH = 3.95

 

12. pOH = 3.65

 

 

13. pOH = 5.07

Equilibrium and Le Chateleir's Principal

Instructions: Write the equilibrium expression for each chemical equation.

 

1.

 

 

2.

 

Oxidation-Reduction Reactions

Instructions: Assign an oxidation state to each element, ion, or molecule.

1. Cl-

2. Br2

3. S-2

4. Fe3+

Instructions: Assign an oxidation state to each atom in each compound.

5.

6.

7.

8.

Instructions: Assign an oxidation state to each atom in each polyatomic ion.

9.

10.

11.

12.

Instructions: Identify the oxidation state of P or Si in each ion.

13.

14.

15.

16.