For the elementary reaction 2A $⇌$ B,The forward and backward rate constants are $k_{1}$ and $k_{2}$ respectively. Then the rate of disappearance of A is equal to:

$k_{1} [A]^{2} - k_{2} [B]$

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$2 k_{1} [A]^{2} + 2 k_{2} [B]$

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$2 k_{1} [A]^{2} - 2 k_{2} [B]$

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$[2 k_{1} - k_{2}] [A]$

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Solution

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

Rate of reaction:
$= - \frac{1}{2} \frac{d [A]}{d t} = k_{1} [A]^{2} - k_{2} [B] ∴ rate of disappearance of A = \frac{- d [A]}{d t} = 2 k_{1} [A]^{2} - 2 k_{2} [B]$

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For the elementary reaction 2A $⇌$ B,The forward and backward rate constants are $k_{1}$ and $k_{2}$ respectively. Then the rate of disappearance of A is equal to:

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For the elementary reaction 2A ⇌ B,The forward and backward rate constants are k1 and k2 respectively. Then the rate of disappearance of A is equal to:

The correct option is C 2k1[A]2−2k2[B] Rate of reaction: =−12d[A]dt=k1[A]2−k2[B]∴rate of disappearance of A=−d[A]dt=2k1[A]2−2k2[B]

For the elementary reaction 2A $⇌$ B,The forward and backward rate constants are $k_{1}$ and $k_{2}$ respectively. Then the rate of disappearance of A is equal to:

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

Rate of reaction:
$= - \frac{1}{2} \frac{d [A]}{d t} = k_{1} [A]^{2} - k_{2} [B] ∴ rate of disappearance of A = \frac{- d [A]}{d t} = 2 k_{1} [A]^{2} - 2 k_{2} [B]$