Question

Increase in temperature favours the equilibrium conversion of:

• A. All reactions
• B. Exothermic reactions
• C. Endothermic reactions
• D. Reversible reactions only

Hint:

Logic Tip: Endothermic means "requires heat." Therefore, if you supply more heat by increasing the temperature, you are feeding the reaction exactly what it needs to move forward and produce more product!

Answer 1

The Correct Option is C

Concept:
Le Chatelier's Principle dictates how a system at equilibrium responds to external changes. When temperature is altered, the system shifts to counteract that specific thermal change.

Step 1: Chemical reactions either release heat to the surroundings (Exothermic, $\Delta H < 0$) or absorb heat from the surroundings (Endothermic, $\Delta H > 0$).

Step 2: For an endothermic reaction, heat acts like a necessary "reactant" to drive the process forward (Reactants + Heat $\rightleftharpoons$ Products).

Step 3: When you increase the temperature, you are essentially adding more "heat" to the system.

Step 4: To counteract the addition of extra heat, the system shifts in the direction that consumes heat.

Step 5: Because endothermic reactions naturally consume heat to proceed, an increase in temperature will drive the equilibrium forward, thereby favouring the conversion of endothermic reactions.