1. Tardigrade
  2. Question
  3. Chemistry
  4. The equilibrium constants for the reaction, Br2 leftharpoons 2 Br → 1 at 500 K and 700 K are 1 × 10-10 and 1 × 10-5 respectively. The reaction is

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. The equilibrium constants for the reaction, $Br_2 \rightleftharpoons 2\,Br \to 1$
at $500 \,K$ and $700 \,K$ are $1 \times 10^{-10}$ and $1 \times 10^{-5}$ respectively. The reaction is

UPSEEUPSEE 2013Equilibrium

Solution:

Chemical equilibrium constant for the reaction is

$Br _{2} \rightleftharpoons 2\, Br$ is

$K_{c}=\frac{[ Br ]^{2}}{\left[ Br _{2}\right]}$

$K_{c}$ at $500 \,K$ is $1 \times 10^{10}$. On increasing temperature $(700 \,K )$. The value of $K_{c}$ is also increased, i.e., concentration of product is increased and obuiously the increase of temperature will favour the forward reaction. Thus. the forward reaction is endothermic.