1. Tardigrade
  2. Question
  3. Chemistry
  4. The rate of the elementary reaction, A2(g)+B2(g) leftharpoons 2 A B(g) is given by rate =1.7 × 10-18[A2][B2] The rate of decomposition of gaseous AB to A2 and B2 is given by rate =2.4 × 10-21[A B]2. The equilibrium constant, for the formation of AB from A2 and B2 is

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Q. The rate of the elementary reaction, $A_{2(g)}+B_{2(g)} \rightleftharpoons 2 A B_{(g)}$ is given by rate $=1.7 \times 10^{-18}\left[A_{2}\right]\left[B_{2}\right]$ The rate of decomposition of gaseous $AB$ to $A_{2}$ and $B_{2}$ is given by rate $=2.4 \times 10^{-21}[A B]_{2}$. The equilibrium constant, for the formation of $AB$ from $A_{2}$ and $B_{2}$ is

Equilibrium

Solution:

$A_{2(g)}+B_{2(g)} \xrightleftharpoons[{k_{b}}] {k_{f}} 2AB_{(g)}$

Rate of forward reaction $\left(r_{f}\right)=k_{f}\left[A_{2}\right]\left[B_{2}\right]$

Rate of backward reaction $\left(r_{b}\right)=k_{b}[A B]^{2}$

$\therefore k_{f}=1.7 \times 10^{-18}, k_{b}=2.4 \times 10^{-21}$

$K=\frac{k_{f}}{k_{b}}=\frac{1.7 \times 10^{-18}}{2.4 \times 10^{-21}}=0.708 \times 10^{3}$