For a reaction $A \xrightarrow{K_1} B \xrightarrow{K_2} C$ If the rate of formation of B is set to be zero then the concentration of B is given by:

The rate of formation of B is: \[ \frac{d[\text{B}]}{dt} = k_1[\text{A}] - k_2[\text{B}]. \] For the rate of formation of B to be zero: \[ \frac{d[\text{B}]}{dt} = 0. \] Substitute: \[ k_1[\text{A}] - k_2[\text{B}] = 0. \] Rearrange to find [B]: \[ k_1[\text{A}] = k_2[\text{B}] \implies [\text{B}] = \frac{k_1}{k_2}[\text{A}]. \] Thus, the concentration of B is: \[ [\text{B}] = \left(\frac{k_1}{k_2}\right)[\text{A}]. \]

For a reaction 1 2 K K A B C; If the rate of formation of B is set to be zero then the concentration of B is given by :

The data provided in the table were obtained from the following reaction, carried out at 273 𝐾.
𝐴 + 𝐵 → 𝐶

Initial concentration of [𝐴] 𝑚𝑜𝑙 $𝐿 ^{−1}$	Initial concentration of [𝐵] 𝑚𝑜𝑙$𝐿 ^{−1}$	Initial rate of formation of [𝐶] 𝑚𝑜𝑙 $𝐿^{−1} 𝑠 ^{−1}$
0.2	0.2	0.3
0.4	0.2	0.6
0.4	0.4	2.4

The order of the reaction with respect to 𝐴 is _________.