Question

In: Chemistry

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g),...

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), ΔH = -206 kJ/mol, state whether the yield of CH4 will increase, decrease or remain the same for the following changes:

Adding some H2 gas to the system

Removing H2O from the system

Increasing the volume of the system

Decreasing the temperature on the system

Adding a catalyst to the system

Solutions

Expert Solution

1)

Adding reactant will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

Answer: Increase

2)

Removing product will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

Answer: Increase

3)

Increasing volume will decrease the pressure which in turn shift the reaction in a direction which have greater gaseous molecules as per Le chatelier Principle

Here reactant has more gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

Answer: decrease

4)

Decreasing Temperature will shift the reaction in a direction which release heat as per Le chatelier Principle

Forward reaction is exothermic in nature

hence, forward reaction will be favoured

So, Equilibrium moves to product side

Answer: Increase

5)

Catalyst doesn't affect equilibrium

So, No effect on equilibrium

Answer: remains the same

queen_honey_blossom answered 2 years ago
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