Question

What does it mean when equilibrium shifts to left?

Answer 1

1. The equilibrium is the condition when all the reactants are consumed to form the products.
2. Equilibrium is established under certain specific conditions that need to be maintained for a longer period of time until the equilibrium is obtained.
3. After obtaining the equilibrium any change in condition will disrupt the equilibrium.
4. To overcome such disruption the equilibrium shifts back to its initial condition and that is signified by Le Chatelier's Principle.
5. This “disruption” can be resolved by adding or subtracting the reactant or product molecule in the chemical reaction.
6. If in case the reactant is added such reaction will shift toward the right side and if products are added then equilibrium shifts to the left side.
7. With the help of a chemical reaction we can understand more clearly how the equilibrium shifts to left.
8. The chemical reaction is as follows.
   ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons \mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right);∆\mathrm{H}=-40\mathrm{KJ}/\mathrm{mol}$
9. The reaction is endothermic in nature because the change in enthalpy is negative and thus the equilibrium shifts to left.