Unit 7 Review - Kinetics and Thermodynamics

The specific heat of water is 4.18J/(g·ºC). How many joules are required to heat 100 grams of water from 25ºC to 35ºC?
1. 4180 J
2. 239 J
3. 14630 J
4. 10450 J
A 5 gram piece of a metal at 0ºC absorbs 1000 J of energy, after which the temperature of the metal is 400ºC. What is the specific heat of the metal?
1. 0.5 J/(g·ºC)
2. 2 J/(g·ºC)
3. 0.25 J/(g·ºC)
4. 2 x 10⁶ J/(g·ºC)
The specific heat of gold is 0.13 J/(g·ºC). How many joules are required to heat 40 grams of gold from 60ºC to 85ºC?
1. 130 J
2. 12.3 J
3. 4.8 J
4. 13 J
Ice has a specific heat of 2 J/(g·ºC). How many joules must be absorbed by a 50 gram piece of ice in order to raise the temperature from -18ºC to -10ºC?
1. 800 J
2. 12.5 J
3. 3.125 J
4. 0.32 J
The molar heat of fusion for water is 6 kJ/mol. How much energy is required to melt 3 moles of ice at 0ºC?
1. 18 kJ
2. 2 kJ
3. 0.50 kJ
4. 9 kJ
The molar heat of fusion for water is 6 kJ/mol. How much energy must be removed from 10 moles of water at 0ºC in order to convert it to ice at 0ºC?
1. 60 kJ
2. 0.6 kJ
3. 1.66 kJ
4. 16 kJ
The molar heat of vaporization for water is 41 kJ/mol. How much energy must be absorbed by 20 moles of water at 100ºC in order to convert it to steam at 100ºC?
1. 820 kJ
2. 4100 kJ
3. 82 000 kJ
4. 8.2 kJ
The process of converting ice to water by occurs by:
1. the addition of energy
2. the removal energy
3. no change in energy
Which of the following is written incorrectly?
1. liquid water + energy --> ice
2. liquid water + energy --> water vapor
3. water vapor --> liquid water + energy
4. ice + energy --> liquid water
Equal masses of each of the following substances absorb an equal amount of energy. Which substance experiences the greatest temperature increase?

Iron; specific heat = 0.449 J/(g·ºC)
Aluminum; specific heat = 0.897 J/(g·ºC)
Liquid water; specific heat = 4.18 J/(g·ºC)
Ice; specific heat = 2.06 J/(g·ºC)
1. Iron
2. Aluminum
3. Liquid water
4. Ice
Which of the following will always increase the rate of a chemical reaction?
1. An increase in pressure
2. An increase in concentration of reactants
3. An increase in temperature
4. A decrease in pressure
An increase in temperature increases the rate of a chemical reaction by what means
1. Increasing the concentration of reactants
2. Increasing pressure
3. Decreasing activation energy
4. Increasing collision energy
5. Increasing collision frequency
Catalysts increase the rate of a chemical reaction by what means?
1. Increasing collision energy
2. Increasing the concentration of reactants
3. Lowering activation energy
4. Increasing temperature
Which of the following will burn most rapidly?
1. Solid alcohol
2. Liquid alcohol
3. Vaporized alcohol
4. All burn at the same rate
In chemical reactions, electricity, a spark, and sunlight are all ways in which _______________ may be provided.
1. activation energy
2. reactants
3. products
4. catalysts
For an effective collision to take place, there must be:
1. A sufficiently hard collision
2. A correctly oriented collision
3. A catalyst present
4. No products present
5. High pressure
Which of the following is guaranteed to slow down the rate of a chemical reaction?
1. Addition of a catalyst
2. Decreasing the temperature
3. Increasing the temperature
4. Decreasing the concentration of the reactants
5. Increasing the pressure
At 25 ºC, a certain reaction is able to produce 0.80 moles of product per minute? At what rate might the product be produced at 35 ºC?
1. 0.40 moles per minute
2. 1.6 moles per minute
3. 0.20 moles per minute
4. 0.80 moles per minute
At 25 ºC, a certain reaction is able to produce 0.80 moles of product per minute? At what rate might the product be produced at 15 ºC?
1. 0.40 moles per minute
2. 1.6 moles per minute
3. 1.20 moles per minute
4. 0.80 moles per minute
In this chemical reaction:

2 HCl(aq) + Mg(s) <--> MgCl₂(aq) + H₂(g) + heat
1. energy is given off, so the reaction is endothermic
2. energy is given off, so the reaction is exothermic
3. energy is absorbed, so the reaction is endothermic
4. energy is absorbed, so the reaction is exothermic
Given the following reaction:

P₄(s) + 5 O₂(g) --> 2 P₂O₅(s)

If the intial rate of the reaction consumes 1 mole of phosphorus, P₄, per second, what is the rate at which oxygen, O₂, is consumed initially?
1. 1 mole per second
2. 2 moles per second
3. 0.2 moles per second
4. 5 moles per second
Given the following reaction:

P₄(s) + 5 O₂(g) --> 2 P₂O₅(s)

If the intial rate of the reaction consumes 1 mole of phosphorus, P₄, per second, what is the rate at which diphosphorus pentoxide, P₂O₅, is formed initially?
1. 1 mole per second
2. 2 moles per second
3. 0.2 moles per second
4. 5 moles per second
Given the following reaction:

C₃H₈(g) + 5 O₂(g) --> 3 CO₂ + 4 H₂O(g)

If the intial rate of the reaction produces 2 moles of water vapor, H₂O, per second, what is the rate at which carbon dioxide, CO₂, is formed initially?
1. 3 moles per second
2. 2 moles per second
3. 2.67 moles per second
4. 1.5 moles per second
Given the following reaction:

C₃H₈(g) + 5 O₂(g) --> 3 CO₂ + 4 H₂O(g)

If the intial rate of the reaction produces 2 moles of water vapor, H₂O, per second, what is the rate at which oxygen, O₂, is consumed initially?
1. 1 mole per second
2. 2 moles per second
3. 8 moles per second
4. 2.5 moles per second
Given the following reaction:

C₃H₈(g) + 5 O₂(g) --> 3 CO₂ + 4 H₂O(g)

If the intial rate of the reaction produces 2 moles of water vapor, H₂O, per second, what is the rate at which propane, C₃H₈, is consumed initially?
1. 1 mole per second
2. 2 moles per second
3. 4 moles per second
4. 0.5 moles per second
Given the following reaction:

2 H₂(g) + O₂(g) --> 2 H₂O

As this reaction takes place:
1. the quantity of water vapor, H₂O(g), decreases
2. the quantities of hydrogen, H₂, and oxygen, O₂, decrease
3. the quantities of hydrogen, H₂, and oxygen, O₂, increase
4. the quantity of hydrogen, H₂, increases and the quantity of oxygen, O₂, decreases
Given the following reaction:

H₂(g) + Cl₂(g) --> 2 HCl

As this reaction takes place:
1. HCl is produced at the same rate that H₂ is consumed
2. H₂ and Cl₂ are consumed at the same rate
3. HCl is produced at the twice the rate that Cl₂ is consumed
4. HCl is produced at the half the rate that Cl₂ is consumed
For the forward reaction depicted in this diagram, DH = ?
1. 10 kJ/mol
2. -20 kJ/mol
3. 65 kJ/mol
4. 30 kJ/mol
5. -30 kJ/mol
For the forward reaction depicted in this diagram, the Activation Energy, E_a = ?
1. 10 kJ/mol
2. 55 kJ/mol
3. -30 kJ/mol
4. -20 kJ/mol
5. 65 kJ/mol
For the reverse reaction depicted in this diagram, DH = ?
1. 10 kJ/mol
2. -20 kJ/mol
3. 65 kJ/mol
4. 30 kJ/mol
5. -30 kJ/mol
For the reverse reaction depicted in this diagram, the Activation Energy,E_a = ?
1. -20 kJ/mol
2. 65 kJ/mol
3. 85 kJ/mol
4. 10 kJ/mol
5. -55 kJ/mol
The forward reaction depicted in this diagram is:
1. Endothermic
2. Exothermic
3. Isothermic
When extra NH₃ is added to the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When N₂ is removed from the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When H₂ is added to the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the pressure is increased on the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the pressure is decreased on the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the temperature is decreased on the following system at equilibrium:

2 HCl(aq) + Mg(s) <--> MgCl₂(aq) + H₂(g) + heat
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the temperature is increased on the following system at equilibrium:

2 HCl(aq) + Mg(s) <--> MgCl₂(aq) + H₂(g) + heat
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the temperature is decreased on the following system at equilibrium:

2 HCl(aq) + Mg(s) <--> MgCl₂(aq) + H₂(g) + heat
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs