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Effect on Kc

For the eleme...

Question

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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Similar questions

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:

Which of the following statement(s) is/are correct about the rate expression?

(K_{1}

and

K_{2}

are reaction constant for forward and backward reaction respectively.

)

Q. In a reaction

A + B ⇌ C + D

, the rate constant of forward reaction and backward reaction is

K_{1}

and

K_{2}

, then the equilibrium constant (K) for reaction is expressed as

Q. The activation energy for forward and backward reactions are

50 k J / m o l

and

40 k J / m o l

respectively. If

K_{1}

and

K_{2}

are the equilibrium constants of reaction at temperature

T_{1}

and

T_{2}

respectively and

T_{2} > T_{1}

then:

Q. The rate constants of a reaction at 300K & 280K respectively are

K_{1}

K_{2}

. Then:

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