| 10 minutes maximum! (can you do it in 5?) |
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1. When a reaction is in dynamic equilibrium the rate of the forward reaction is
the rate of the reverse reaction. |
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2.
When a reaction is in dynamic equilibrium the concentrations of the reactants and products are always….
- A. equal
- B. unequal with the reactant concentration greater than the product concentration
- C. unequal with the product concentration greater than the reactant concentration
- D. constant
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3. The reaction of anhydrous copper(II)sulfate with water is an example of a reversible reaction:
| CuSO4 (s) |
+ |
5H2O
(l) |
⇌ |
CuSO4.5H2O
(s) |
| white |
|
|
|
blue |
|
-sulfate.jpg) |
If the reaction moves in the forward direction you will observe …..
- A. solid turning from white to blue
- B. solid dissolving
- C. solid turning from blue to white
- D. condensation forming on the sides of the test tube
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Q4-5
The production of ammonia in the Haber Process is an example of a reversible reaction:
| N2 (g) |
+ |
3H2 (g) |
⇌ |
2NH3 (g) |
ΔH = - 92.4kJ |
Select the answer which states and gives a reason for the effect on the yield of ammonia (NH3) of … |
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4. …..increasing the temperature:
| |
Yield of Ammonia |
Reason |
| A |
increases |
because the forward reaction is endothermic |
| B |
increases |
because the reverse reaction is endothermic |
| C |
decreases |
because the forward reaction is endothermic |
| D |
decreases |
because the reverse reaction is endothermic |
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5. …..increasing the pressure:
| |
Yield of Ammonia |
Reason |
| A |
increases |
because there are less moles of gas on the ‘products’ side |
| B |
increases |
because there are less moles of gas on the ‘reactants’ side |
| C |
decreases |
because there are less moles of gas on the ‘products’ side |
| D |
decreases |
because there are less moles of gas on the ‘reactants’ side |
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| 6. The decomposition of dinitrogen tetroxide is an endothermic process as bonds are broken.
This is also a reversible reaction and the equation for this reaction is:
What would be the effect on the position of equilibrium of increasing the temperature and of increasing the pressure? |
 |
| |
Increasing the temperature |
Increasing the pressure |
| A |
Moves to the left |
Moves to the left |
| B |
Moves to the left |
Moves to the right |
| C |
Moves to the right |
Moves to the left |
| D |
Moves to the right |
Moves to the right |
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| 7. Hydrogen and chlorine react in a reversible reaction to produce hydrogen chloride:
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| If the pressure is increased on this equilibrium system, what will happen to the equilibrium position? |
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8. To achieve a high yield (of SO3), what conditions of temperature and pressure would be required?
| 2SO2 |
+ |
O2 |
⇌ |
2SO3 |
ΔH = -385 kJ |
|
|
| |
Temperature |
Pressure |
| A |
low |
low |
| B |
low |
high |
| C |
high |
low |
| D |
high |
high |
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Q9-10:
Hydrogen is produced in industry by reacting methane with steam at 2 atm pressure and 1000 °C. The equation for the reaction is:
| CH4 (g) |
+ |
H2O (g) |
⇌ |
CO (g) |
+ |
3H2 (g) |
ΔH= +210 kJ |
What is the effect on the concentrations of carbon monoxide and hydrogen in the equilibrium mixture of carrying out the reaction at …… |
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9. ………….. 500oC?
| |
Carbon Monoxide Concentration |
Hydrogen Concentration |
| A |
increases |
decreases |
| B |
increases |
increases |
| C |
decreases |
decreases |
| D |
decreases |
increases |
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10. …….10atm?
| |
Carbon Monoxide Concentration |
Hydrogen Concentration |
| A |
increases |
decreases |
| B |
increases |
increases |
| C |
decreases |
decreases |
| D |
decreases |
increases |
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