Question

For the endothermic reaction CACO3(s) CaO(s) +CO2(8) Le Chatelier's principle predicts that will result in an increase in the number of moles of CO2. increasing the temperature decreasing the temperature increasing the pressure removing some of the CaCO3 (s) none of these

Answer 1

Option 1)

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is endothermic in nature

hence, forward reaction will be favoured

So, Equilibrium moves to product side and hence mol of CO2 will increase

Option 2)

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

Forward reaction is endothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

Option 3)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here reactant has less gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

Option 4)

Removing solid or liquid doesn't affect equilibrium

So, No effect on equilibrium

Answer: option 1