Download Chemistry Study Guide

Chemistry
Name
Period
Chemistry Study Guide
Chapter 9 Stoichiometry
1.
2.
3.
4.
5.
a)
b)
1.
2.
3.
4.
5.
6.
7.
8.
1.
2.
3.
4.
5.
6.
7.
8.
1.
2.
3.
What is a limiting reagent? How do you find the mole ratio for reactants and products in a stoichiometry problem?
Calculate the mass of silver needed to react with chlorine to produce 84.0 g of silver (I) chloride. Write a balanced equation.
What mass of ammonia, NH3, is necessary to react with 2.1 x 1024 molecules of oxygen in the following equation?
___NH3(g) +___ O2(g)
___H2O(g) + ___NO2(g)
Calculate the percent yield in the electrolytic decomposition of hydrogen chloride if 25.8 g of HCl produce 13.6 g of chlorine gas.
__ HCl(aq)
_ H2(g) + _ Cl2(g)
Water can be made by cooling 16.2 g of hydrogen gas and 16.4 g of oxygen gas.
___H2 (g) + ___O2(g)
___H2O(l)
What is the limiting reagent?
What is the maximum amount of water that can be synthesized?
Chapter 10 States of Matter
State the 5 basic assumptions of the kinetic molecular theory.
What is the relationship between the temperature, speed and kinetic energy of gas molecules?
Explain how the attractive forces between particles in a liquid are related to the equilibrium vapor pressure of that liquid.
What is the relationship between atmospheric pressure and the boiling point of a liquid?
Water has a high heat of fusion (6.009 KJ/mol) and a high heat of vaporization (40.79 KJ/mol). Explain what this means in
terms of attraction between particles.
Using the values given in #5, Is this an exothermic or endothermic reaction?
Explain why the water molecule is polar. In your explanation, include why the water molecule is bent?
Describe how the intermolecular forces in water allow for each of the following properties of water:
a. low vapor pressure
c. solid H2O is less dense than liquid H2O
b. high heat of vaporization
d. high boiling point for a molecule of its mass
Chapter 11 Gases
Explain what happens to the pressure inside a balloon when you blow into it.
Why can’t an ideal gas be liquefied?
What would be the number of moles and grams of carbon dioxide gas contained in an 855 mL container at 35˚C and 1860
mmHg of pressure?
If a 2.75 L container of gas at 24.0˚C and 95.2 kPa was compressed to 1820 mL and warmed to 40.0˚C, what would be the new
pressure?
A mixture of 3 gases, A,B and C, is at a total pressure of 6.11 atm. The partial pressure of A is 168 kPa and B is 3.89 atm. What
is the partial pressure of gas C?
Ammonia and ethanol are released at the same time across a room. Which will you smell first?
What is the volume of 8.00 grams of oxygen at STP?
Explain the differences in Charle, Boyle and Gay Lussac’s Laws from the combined gas law.
Chapter 16 Thermochemistry
How much heat, does 32.0 g of water absorb when it is heated from 25ºC to 80ºC? How many joules is this?
The temperature of a piece of copper with a mass of 95.4 g changes from 25.0ºC to 48.0ºC when the metal absorbs 849 J of
heat. What is the specific heat of copper? Is this an exothermic or endothermic reaction?
Will the specific heat of 50.0 g of a substance be the same as or greater than the specific heat of 10.0 g of the same substance?
5.
Write the Enthalpy of formation for the reaction of W(s) + C(s)  WC(s) using the reaction steps below
2W(s) + 3O2  2WO3; ∆H = -842.9kJ
C(s) + O2(g)  CO2(g); ∆H = -393.5kJ
2WC(s) + 5O2(g)  2WO3(s) + 2CO2(g); ∆H = -2391.8kJ
6. What is the enthalpy for the reaction of CO 2(g) + 2Mg(s)  2MgO(s) + C(s) ?
1.
2.
3.
4.
5.
1.
2.
3.
4.
5.
6.
7.
8.
1.
2.
3.
4.
Chapter 12 Solutions
Define the following terms:
a. solubility
b. saturated solution
c. unsaturated solution
d. Henry’s law
How does each of the following affect the solubility of (a) a solid dissolved in a liquid, and (2) a gas dissolved in a liquid.
a. an increase in temperature
c. an increase in pressure
b. shaking, agitation
d. an increase in pressure with a decrease in temperature
Differentiate between the following:
a. a dilute unsaturated solution and a dilute saturated solution
b. a concentrated saturated solution and a concentrated unsaturated solution
c. a supersaturated solution and saturated solution
Calculate the following (SHOW ALL WORK):
a. The molarity of a solution containing 42.6g of sodium hydroxide in 3.00L of water.
b. The number of moles of solute present in 680mL of a 0.25M Na2SO4 solution.
c. The number of grams of KBr present in 500mL of a 0.100 M solution.
Describe how to prepare the following solutions. Include calculations, a description of the procedure, and specific equipment.
a. 400.0 mL of 0.15 M solution of copper (II) sulfate from 0.75M stock solution.
b. 50.0 mL of a 0.20 M solution of potassium nitrate from a 4.0 M stock solution.
Chapters 17-18 Rates of Reaction and Equilibrium
Define the following terms:
a. activation energy
c. chemical equilibrium
e. Le Chatelier’s principle
b. catalyst
d. collision theory
f. reaction mechanism
Draw energy diagrams and label the reactants, products, activated complex, activation energy, and energy change for:
a. an exothermic reaction
b. and endothermic reaction
c. a reaction with and without the presence of a catalyst
Use the collision theory to explain how and why each of the following affects the rate of a reaction:
a. an increase in temperature
c. surface area
b. a decrease in the concentration of a reactant
d. use of a catalyst
Predict how each of the following changes will affect the equilibrium position of the given reaction:
PCl5(g)
PCl3(g) + Cl2(g) + energy
a. increase the pressure
c. decrease the amount of Cl2
e. increase the volume of the container
b. decrease the temperature
d. add more PCl5 to the reaction vessel
Write the rate law for the following reaction and solve for the specific rate constant. What is the order for each reaction in terms
of A, B and the overall reaction.
3A + 4B
 A3B4
Experiment #
[A]
[B]
Rate of reaction M/s
1
2.0
5.0
3.0 x 10-4
2
4.0
5.0
1.2 x 10-3
3
2.0
10.0
1.2 x 10-3
Write the equilibrium constant expression for each of the following reactions: (NOTE – you must first balance the equations!)
a. NH3 (g) + O2 (g)
NO (g) + H2O (g)
c. COCl2 (aq)
CO (g) + Cl2 (g)
b. N2O4 (g)
NO2 (g)
d. CaO (s) + CO2 (g)
CaCO3(s)
For each of the following reactions, determine whether the reactants or the products are favored:
a. H2Cr2O7 (aq) + 4 NaOH (aq)
2 Na2CrO4 (aq) + 3 H2O(l)
Keq = 5.62 x 1049
b. N2 (g) + O2 (g)
2NO (g)
Keq = 1.2 x 10-4
Calculate Keq for the following general equations, given the concentration provided:
a. 2 A + B
2C
[A] = 0.6M
[B] = 0.1M
[C] = 0.4 M
b. A + 3B
C
[A] = 1.2M
[B] = 0.4M
[C] = 0.2 M
c. For the reactions above, are the products or the reactants favored?
Chapter 13-Ions in Aqueous Solutions and Solubility
Differentiate between strong electrolytes, weak electrolytes, and nonelectrolytes. Give two examples of each and explain why
you placed them in each category.
Predict the solubility of each of the following substances in: (1)water and (2) heptanes
a. sodium iodide
c. hydrogen bromide
e. ethanol
g. tetra chloromethane
b. nickel (solid)
d. calcium carbonate
f. benzene
Why do you believe each of the above is or isn’t soluble in the solvents mentioned?
Write the overall ionic equation, and net ionic equation for the precipitation reaction of Ca(OH) and NaCO3. (use you solubility
table page 437)
Chapter 14 and 15 Acids and Bases, Neutralization and Titration
List at least three properties of acids and three properties of bases.
Differentiate between Arrhenius, Bronsted-Lowry, and Lewis acids and bases. Give an example of each.
For the following reaction, label the acid, base, conjugate acid, and conjugate base. List the conjugate acid-base pairs.
CH3COOH + H2O
CH3COO- + H3O+
4. Calculate the following:
a. [OH] when [H+] of a solution is .0024 M
c. pH of a .025M solution of HCl e. pH of a 2.20M solution of Ca(OH)2
b. [H+] when [KOH] is 1.6 x 10-12M
d. pOH of a .025M solution of HCl
5. Show the balanced equation for the self-ionization of water. What is the pH at 25oC?
6. Differentiate between the following and give an example of each:
a. strong acids and weak acids
b. strong bases and weak bases
7. Explain how it is possible to have:
a. a concentrated weak acid
b. a dilute strong acid
8. Predict the products for the following acid-base reactions & write balanced equations.
a. hydrochloric acid + sodium hydroxide
c. ammonia + sulfuric acid
b. carbonic acid + calcium hydroxide
d. ethanoic acid + potassium hydroxide
9. Calculate the following:
a. The number of moles of NaOH needed to neutralize 3.5 moles of HCl
b. The number of moles of HCl needed to neutralize 6.0 moles of Mg(OH) 2 (watch your mole ratios)
10. Calculate the following:
a. [HCl ] if 2.0 mL was needed to neutralize 40.0 mL of a 0 .20M NaOH solution
b. Number of moles of Mg(OH)2 present in 50.0 mL of solution, if 75.0 mL of a 0.1 M HCl solution was needed to reach the
equivalence point
c. The molarity of a NaOH solution, if 20.0 mL of the solution was neutralized by 28.0 mL of a 1.0 M H 3PO4 solution
1.
2.
3.