For the reaction, H2(g)+Br2(g) arrow 2HBr(g), the reaction rate =k[H2] [Br2]1 /2. Which statement is true about this reaction?

Question

For the reaction, H2(g)+Br2(g) arrow 2HBr(g), the reaction rate =k[H2] [Br2]1 /2. Which statement is true about this reaction? (A) The reaction is of second order. (B) Molecularity of the reaction is 3/2. (C) The unit of k is sec-1 . (D) Molecularity of the reaction is 2.

Tardigrade Admin · Accepted Answer

Explanation: H 2(g)+ Br 2(g) longrightarrow 2 HBr (g) The molecularity of the reaction is 1+1=2 Rate of reaction =K[H2][B r2]1 / 2 Order of reaction =1+(1/2)=(3/2) Unit of K=mol-1 / 2 L1 / 2 s-1

Q. For the reaction, $H_{2 (g)} + B r_{2 (g)}$ $\to$ $2 H B r (g)$ , the reaction rate $= k [H_{2}]$ $[B r_{2}]^{1/2}$ . Which statement is true about this reaction?

The reaction is of second order.

Molecularity of the reaction is 3/2.

The unit of $k$ is $se c^{- 1}$ .

Molecularity of the reaction is 2.

Explanation:
$H_{2} (g) + B r_{2} (g) ⟶ 2 H B r (g)$
The molecularity of the reaction is $1 + 1 = 2$
Rate of reaction $= K [H_{2}] [B r_{2}]^{1/2}$
Order of reaction $= 1 + \frac{1}{2} = \frac{3}{2}$
Unit of $K = m o l^{- 1/2} L^{1/2} s^{- 1}$

Q. For the reaction, H2(g)​+Br2(g)​ → 2HBr(g), the reaction rate =k[H2​] [Br2​]1/2. Which statement is true about this reaction?