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Use the endothermic reaction below to answer the following questions: C(s) + H2O(g) <------> CO(g) +...

Use the endothermic reaction below to answer the following questions:

C(s) + H2O(g) <------> CO(g) + H2(g)

Decide how the reaction shifts (to reactants, to products, or no shift) based on each of the following disturbances below

1. The volume of the container is halved.

2. The temperature of the system is increased.

3. CO (g) is removed.

4. A catalyst is added.

5. Additional C(s) is added.

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Answer #1

C(s) + H2O(g) <------> CO(g) + H2(g)

1. The volume of the container is halved.

reaction shifts to product side

2. The temperature of the system is increased.

reaction shifts to product side

it is endothermic reaction. so temperature increase favours the forward direction. that is product side

3. CO (g) is removed.

reaction shifts to product side

if products are removed equilibrium shifts to product side.

4. A catalyst is added.

no shift

catalyst does not effect the equilibrium

5. Additional C(s) is added.

no shift

it is solid. so no effect on the equilibrium. pure solids and liquids have no effect on equilibrium constant

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