For an elementary chemical reaction,
the expression for $\frac{d [A]}{d t}$ is

2 k_{1} [A_{2}] - 2 k_{- 1} [A]^{2}

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k_{1} [A_{2}] - k_{- 1} [A]^{2}

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k_{1} [A_{2}] + k_{- 1} [A]^{2}

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2 k_{1} [A_{2}] - k_{- 1} [A]^{2}

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Solution

The correct option is A $2 k_{1} [A_{2}] - 2 k_{- 1} [A]^{2}$

$- \frac{1}{2} \frac{d [A]}{d t} = k_{- 1} [A]^{2} - k_{1} [A_{2}]$
$\frac{d [A]}{d t} = - 2 k_{- 1} [A]^{2} + 2 k_{1} [A_{2}]$
$\Rightarrow \frac{d [A]}{d t} = 2 k_{1} [A_{2}] - 2 k_{- 1} [A]^{2}$

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For an elementary chemical reaction, the expression for d[A]dt is

The correct option is A 2k1[A2]−2k−1[A]2 −12d[A]dt=k−1[A]2−k1[A2] d[A]dt=−2k−1[A]2+2k1[A2] ⇒d[A]dt=2k1[A2]−2k−1[A]2

For an elementary chemical reaction,
the expression for $\frac{d [A]}{d t}$ is

The correct option is A $2 k_{1} [A_{2}] - 2 k_{- 1} [A]^{2}$

$- \frac{1}{2} \frac{d [A]}{d t} = k_{- 1} [A]^{2} - k_{1} [A_{2}]$
$\frac{d [A]}{d t} = - 2 k_{- 1} [A]^{2} + 2 k_{1} [A_{2}]$
$\Rightarrow \frac{d [A]}{d t} = 2 k_{1} [A_{2}] - 2 k_{- 1} [A]^{2}$