For a reaction A xrightarrowK_1 ~B xrightarrowK_2 C If the rate of formation of B is set to be zero then the concentration of B is given by :

Correct answer: (B) (K_1 / K_2 )[A]. Rate of formation of B is (d[B])/dt=k_1[~A]-k_2[~B] 0=k_1[~A]-k_2[~B] (k_1/k_2 )[A]=[B]

Q12 / 90 · JEE Main 2024 (08 Apr Shift 2) · Chemistry

For a reaction $\mathrm{A} \xrightarrow{\mathrm{K}_1} \mathrm{~B} \xrightarrow{\mathrm{K}_2} \mathrm{C}$ If the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by :

A
$\left(\mathrm{K}_1+\mathrm{K}_2\right)[\mathrm{A}]$
Correct answer
B
$\left(\mathrm{K}_1 / \mathrm{K}_2\right)[\mathrm{A}]$
C
$\left(\mathrm{K}_1-\mathrm{K}_2\right)[\mathrm{A}]$
D
$\mathrm{K}_1 \mathrm{~K}_2[\mathrm{~A}]$

Solution

Rate of formation of $B$ is $\begin{aligned} & \frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}=\mathrm{k}_1[\mathrm{~A}]-\mathrm{k}_2[\mathrm{~B}] \\ & 0=\mathrm{k}_1[\mathrm{~A}]-\mathrm{k}_2[\mathrm{~B}] \\ & \left(\frac{\mathrm{k}_1}{\mathrm{k}_2}\right)[\mathrm{A}]=[\mathrm{B}]\end{aligned}$

Hence, the correct answer is option: 'B'.

For a reaction \(\mathrm{A} \xrightarrow{\mathrm{K}_1} \mathrm{~B} \xrightarrow{\mathrm{K}_2} \mathrm{C}\) If the rate of formation of \(B\) is set to be zero then the concentration of \(B\) is given by :

Solution

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