Consider the following single step reaction in gas phase at constant temperature 2A(g) + B(g) → C(g)

Question

Consider the following single step reaction in gas phase at constant temperature

\(2A _{(g)} + B _{(g)} \rightarrow C _ {(g)}\)

The initial rate of the reaction is recorded as \(r_1\)when the reaction starts with 1.5 atm pressure of A and 0.7 atm pressure of B. After some time, the rate \(r_2\) is recorded when the pressure of C becomes 0.5 atm. The ratio \(r _ 1 : r_2\) is ____ \(\times 10 ^{-1}.\) (Nearest integer)

Answer 1

Correct answer is : 315

2A(g) + B(g) \(\rightarrow\) C(g)

\(r_1\) 1.5 atm 0.7 atm

\(r_2\) 0.5 atm 0.2 atm 0.5 atm

\(\because \mathrm{r}=\mathrm{K}\left[\mathrm{P}_{\mathrm{A}}\right]^2\left[\mathrm{P}_{\mathrm{B}}\right] \)

\(\mathrm{r}_1=\mathrm{K}[1.5]^2[0.7] \)

\( \mathrm{r}_2=\mathrm{K}[0.5]^2[0.2]\)

\(\frac{\mathrm{r}_1}{\mathrm{r}_2}=9 \times \frac{7}{2}=31.5=315 \times 10^{-1}\)