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

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 (A) endothermic (B) exothermic (C) fast (D) slow

Tardigrade Admin · Accepted Answer

Chemical equilibrium constant for the reaction is

B r_{2} ⇌ 2 B r

is

K_{c} = \frac{[ B r ] ^{2}}{[ B r _{2} ]}

K_{c}

at

500 K

is

1 \times 1 0^{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.

Q. The equilibrium constants for the reaction, Br2​⇌2Br→1 at 500K and 700K are 1×10−10 and 1×10−5 respectively. The reaction is

endothermic

exothermic

fast

slow

Q. The equilibrium constants for the reaction, $B r_{2} ⇌ 2 B r \to 1$
at $500 K$ and $700 K$ are $1 \times 1 0^{- 10}$ and $1 \times 1 0^{- 5}$ respectively. The reaction is