Question

The equilibrium constants for the reaction, ${Br}_2\rightleftharpoons 2Br$ at $500K$ and $700K$ are $1\times {10}^{-10}$ and $1\times {10}^{-5}$ respectively. The reaction is:

• A. Endothermic
• B. Exothermic
• C. Fast
• D. Slow

Answer 1

Answer: (A)

Endothermic

The equilibrium constants for the reaction, ${Br}_2\rightleftharpoons 2Br$ at $500K$ and $700K$ are $1\times {10}^{-10}$ and $1\times {10}^{-5}$ respectively. The reaction is endothermic.
An endothermic reaction is characterized by absorption of heat. When heat is added, the position of the equilibrium shifts to forward direction. With increase in temperature, the value of the equilibrium constant increases for an endothermic reaction and decreases for exothermic reaction (Refer image).