Unit 5 Review

The line that represents the activation energy (E_a) of this reaction is
1. Line A
2. Line B
3. Line C
4. Line D
5. Line E
The line that represents the heat of reaction (ΔH, or ΔE) of this reaction is
1. Line A
2. Line B
3. Line C
4. Line D
5. Line E
The heat of reaction (ΔH, or ΔE) of this reaction is
1. 80 kJ
2. -80 kJ
3. 160 kJ
4. 240 kJ
5. -160 kJ
The activation energy (E_a) of this reaction is
1. 160 kJ
2. 80 kJ
3. 240 kJ
4. 40 kJ
5. - 80 kJ
In the reaction depicted in the diagram above,
1. the energy content of the reactants is greater than the energy content of the products
2. the energy content of the products is greater than the energy content of the reactants
3. the energy content of the reactants is the same as the energy content of the products
If you were holding in your hand a test tube in which the reaction above is taking place, it would
1. feel cold, because energy is being absorbed
2. feel hot, because energy is being absorbed
3. feel cold, because energy is being released
4. feel hot, because energy is being released
If a catalyst were added to this reaction, which lines would change?
1. Line A
2. Line B
3. Line C
4. Line D
5. Line E
The line that represents the activation energy (E_a) of this reaction is
1. Line A
2. Line B
3. Line C
4. Line D
The line that represents the heat of reaction (ΔH, or ΔE) of this reaction is
1. Line A
2. Line B
3. Line C
4. Line D
The heat of reaction (ΔH, or ΔE) of this reaction is
1. 80 kJ
2. -80 kJ
3. 160 kJ
4. 240 kJ
5. -160 kJ
The activation energy (E_a) of this reaction is
1. 160 kJ
2. 80 kJ
3. 240 kJ
4. 40 kJ
5. - 80 kJ
In the reaction depicted in the diagram above,
1. the energy content of the reactants is greater than the energy content of the products
2. the energy content of the products is greater than the energy content of the reactants
3. the energy content of the reactants is the same as the energy content of the products
If you were holding in your hand a test tube in which the reaction above is taking place, it would
1. feel cold, because energy is being absorbed
2. feel hot, because energy is being absorbed
3. feel cold, because energy is being released
4. feel hot, because energy is being released
If a catalyst were added to this reaction, which lines would change?
1. Line A
2. Line B
3. Line C
4. Line D
The reaction whose energy diagram is shown here is
1. endothermic
2. exothermic
3. isothermic
The reaction whose energy diagram is shown here is
1. endothermic
2. exothermic
3. isothermic
Which of the following will increase the rate of a chemical reaction?
1. An increase in pressure of gases
2. An increase in concentration of reactants
3. An increase in temperature
4. A decrease in surface area of reactants
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
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 will slow down the rate of a chemical reaction?
1. Addition of a catalyst
2. Decreasing the temperature
3. Increasing the concentration of reactants
4. Increasing the surface area 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
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 the quantity of oxygen, O₂, decreases
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
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
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
The system depicted here is maintained at a temperature of 30 degrees celsius. If the temperature of the system is doubled, the system will achieve equilibrium by which of the following responses?
1. A higher percentage of the water vapor in the container will condense to liquid.
2. A higher percentage of the water will move into the vapor phase.
3. The temperature of the liquid water will exceed the temperature of the vapor.
4. The temperature of the vapor will exceed the temperature of the liquid water.
When the temperature is increased on a closed system containing water and its vapor at equilibrium:

H₂O(l) + heat ⇌ H₂O(g)
1. In order to restore equilibrium, more liquid water evaporates
2. In order to restore equilibrium, water vapor condenses to form liquid water
3. No change occurs
When the temperature is decreased on a closed system containing water and its vapor at equilibrium:

H₂O(l) + heat ⇌ H₂O(g)
1. In order to restore equilibrium, more liquid water evaporates
2. In order to restore equilibrium, water vapor condenses to form liquid water
3. No change occurs
When the pressure is decreased on a closed system containing water and its vapor at equilibrium:

H₂O(l) + heat ⇌ H₂O(g)
1. In order to restore equilibrium, more liquid water evaporates
2. In order to restore equilibrium, water vapor condenses to form liquid water
3. No change occurs
When the pressure is increased on a closed system containing water and its vapor at equilibrium:

H₂O(l) + heat ⇌ H₂O(g)
1. In order to restore equilibrium, more liquid water evaporates
2. In order to restore equilibrium, water vapor condenses to form liquid water
3. No change occurs
The process of dissolving Na₂SO₄ in water is known to be exothermic:

Na₂SO₄(s) ⇌ 2 Na⁺(aq) + SO₄^2-(aq) + heat

If the temperature of the solution is decreased, Na₂SO₄ becomes:
1. More soluble
2. Less soluble
3. No change in solubility occurs
The process of dissolving Na₂SO₄ in water is known to be exothermic:

Na₂SO₄(s) ⇌ 2 Na⁺(aq) + SO₄^2-(aq) + heat

As the temperature of the solution increases, Na₂SO₄ becomes:
1. More soluble
2. Less soluble
3. No change in solubility occurs
This is the aqueous iron(III) thiocyanate equilibrium:

Fe³⁺(yellow) + SCN^-(colorless) ⇌ [FeSCN]²⁺(dark red)

If aqueous iron(III) chloride is added to the solution at equilibrium:
1. The solution becomes colorless
2. The solution becomes more yellow
3. The solution turns darker red
4. No change in color occurs
This is the aqueous iron(III) thiocyanate equilibrium:

Fe³⁺(yellow) + SCN^-(colorless) ⇌ [FeSCN]²⁺(dark red)

If aqueous potassium thiocyanate is added to the solution at equilibrium:
1. The solution becomes colorless
2. The solution becomes more yellow
3. The solution turns darker red
4. No change in color occurs
A beaker with a mixture of ice and water is maintained at equilibrium:

H₂O(s) + heat ⇌ H₂O(l)

If the temperature of the system is increased:
1. Ice melts to form liquid water (shift to the right)
2. Water freezes to form ice (shift to the left)
3. No change occurs
A beaker with a mixture of ice and water is maintained at equilibrium:

H₂O(s) + heat ⇌ H₂O(l)

If the temperature of the system is decreased:
1. Ice melts to form liquid water (shift to the right)
2. Water freezes to form ice (shift to the left)
3. No change occurs
A precipitation reaction achieves equilibrium:

BaCl₂(aq) + Na₂SO₄(aq) ⇌ 2 NaCl(aq) + BaSO₄(s)

If barium chloride (BaCl₂) is added to the system, which change occurs?
1. The reaction shifts to the right, and more precipitate is produced
2. The reaction shifts to the left, and some precipitate dissolves
3. No change occurs