Question

The energy profile diagrams of two reactions are shown in the figure. Then:

• A. reaction A $\to$ B is faster than and more exothermic than reaction C $\to$ D
• B. reaction C $\to$ D is faster than reaction A $\to$ B but less exothermic
• C. reaction C $\to$ D is faster and more exothermic than the reaction A $\to$ B.
• D. reaction C $\to$ D 2.5 times faster than reaction A $\to$ B at the same temperature

Answer 1

The correct option is C reaction C $\to$ D is faster and more exothermic than the reaction A $\to$ B.

Activation energy is defined as the minimum energy required to start a chemical reaction.

Reaction C →D is faster than A→B as it requires less activation energy

The difference in final energy and initial energy is the heat released during the reaction (exothermic/endothermic)

Both reactions are Exothermic. But since difference in initial energy and final energy of C & D is more as compared to A & B, C → D is more exothermic.

Option C is correct.