For the reaction $H_{2} + B r_{2} \to 2 H B r$ overall order is found to be $\frac{3}{2}$ . The rate of reaction can be expressed as:

[H_{2}] [B r_{2}]^{\frac{1}{2}}

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[H_{2}]^{\frac{1}{2}} [B r_{2}]

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[H_{2}]^{\frac{3}{2}} [B r_{2}]^{0}

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All of these

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Solution

The correct option is D All of these
The Order of the Reaction is the sum of powers of the Reactants Concentration in Rate Equation.

So the sum of powers in all the 3 Options is $\frac{3}{2}$ .
Option D is correct

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Similar questions

H_{2} + B r_{2} \to 2 H B r

H_{2} + {B r}_{2} ⟶ 2 H B r

= K [H_{2}] {[{B r}_{2}]}^{\frac{1}{2}}

H_{2} + {B r}_{2} \to 2 H B r

\frac{d x}{d t} = k [H_{2}] {[{B r}_{2}]}^{1 / 2}

H_{2} + {B r}_{2} \to 2 H B r

\frac{d x}{d t} = k [H_{2}]^{1 / 2} {[{B r}_{2}]}^{1 / 2}

{B r}_{2}

H_{2} + B r_{2} \to 2 H B r

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