For a chemical reaction $\mathrm{A}+\mathrm{B} \rightarrow$ Product, the order is 1 with respect to $\mathrm{A}$ and $\mathrm{B}$.
| $\mathrm{Rate}$ $\mathrm{mol~L^{-1}~S^{-1}}$ |
$\mathrm{[A]}$ $\mathrm{mol~L^{-1}}$ |
$\mathrm{[B]}$ $\mathrm{mol~L^{-1}}$ |
|---|---|---|
| 0.10 | 20 | 0.5 |
| 0.40 | $x$ | 0.5 |
| 0.80 | 40 | $y$ |
What is the value of $x$ and $y$ ?
Solution
$$
\begin{aligned}
& \mathrm{r}=\mathrm{K}[\mathrm{A}]^1[\mathrm{~B}]^1 \\\\
& 0.1=\mathrm{K}(20)^1(0.5)^1 ........(i) \\\\
& 0.40=\mathrm{K}(\mathrm{x})^1(0.5)^1 ........(ii) \\\\
& 0.80=\mathrm{K}(40)^1(\mathrm{y})^1 ........(iii)
\end{aligned}
$$
<br/><br/>From (i) and (ii)
<br/><br/>$x=80$
<br/><br/>From (i) and (iii)
<br/><br/>$y=2$
About this question
Subject: Chemistry · Chapter: Chemical Kinetics · Topic: Rate of Reaction
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