At equilibrium, if the rate of the forward reaction increases, the rate of the reverse reaction...
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increases until it is going at the same rate as the forward reaction
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decreases until both reactions are going at the same rate
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carries on at a steady rate
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increases to faster than the forward reaction
Q.2.
What effect will adding a catalyst have to the equilibrium of a system?
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No effect, it just speeds up getting to the point of equilibrium
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It will increase the rate of the forward reaction only
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It will increase the rate of the reverse reaction only
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It decreases the amount of product produced
Q.3.
How do we represent a reversible reaction symbolically?
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→
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←
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↓
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⇌
Q.4.
A stable equilibrium can be achieved in a...
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chemical system
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open system
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closed system
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reaction system
Q.5.
At the point of equilibrium...
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the rate of the forward reaction is greater than the rate of the reverse reaction
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the rate of the forward reaction is slower than the rate of the reverse reaction
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the rate of the forward reaction is double the rate of the reverse reaction
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the rate of the forward reaction is the same as the rate of the reverse reaction
Q.6.
What is a reversible reaction?
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A reaction which will proceed in the forwards direction only
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A reaction which will proceed in both forwards and backwards directions
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A reaction which will proceed in the backwards direction only
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A reaction which will not proceed in any direction
Q.7.
If a reversible reaction is exothermic in the forward direction, in the reverse direction it will be...
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endothermic
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exothermic
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unknown - you cannot tell
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slower
Q.8.
The Haber process is a reversible reaction. If the reaction were at equilibrium, hydrogen and nitrogen would be being produced as quickly as ammonia gas was being broken down. How is the forward reaction rate increased?
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By removing nitrogen and hydrogen from the reaction vessel
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By removing ammonia from the reaction vessel
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By increasing the amount of hydrogen and nitrogen in the reaction vessel
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By increasing the pressure
Q.9.
One example of a reversible reaction is the Haber process. Pick the correct symbol equation for the reaction between hydrogen and nitrogen to produce ammonia in the Haber process.
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N2 + 3H2 → 2NH3
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N2 + 3H2 ← 2NH3
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N2 + 3H2 ⇌ 2NH3
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N2 + 3H2 ⇌ NH3
Q.10.
At equilibrium, the amount of product(s) and reactant(s) is constant. Which of the following would increase the amount of product in a reaction?
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Remove the product from the reaction vessel
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Add more product to the reaction vessel
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Increase the temperature of the reaction mixture
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Increase the pressure of the reaction vessel
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