Medium
The experimental data for the reaction $2A + B_2 \to 2AB$ is given below. Determine the rate equation for the reaction.
$Exp.$ $[A]_0$ $[B_2]_0$ $Rate \ (mol \ L^{-1} \ s^{-1})$ $(1)$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $(2)$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $(3)$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
| $Exp.$ | $[A]_0$ | $[B_2]_0$ | $Rate \ (mol \ L^{-1} \ s^{-1})$ |
| $(1)$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $(2)$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $(3)$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
- A$Rate = k [B_2]$
- B$Rate = k [B_2]^2$
- C$Rate = k [A]^2 [B_2]^2$
- D$Rate = k [A]^2 [B_2]$
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Similar Questions
The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
Difficult
View SolutionWhat is the order and molecularity respectively for the elementary reaction given below?
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$
For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?
Medium
View SolutionThe following results have been obtained during the kinetic studies of the reaction: $2 \ NO + 2 \ H_2 \longrightarrow N_2 + 2 \ H_2O$
Expt $\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$ $[NO] \ (mol \ L^{-1})$ $[H_2] \ (mol \ L^{-1})$ $1$ $4.8 \times 10^{-5}$ $1 \times 10^{-2}$ $1 \times 10^{-3}$ $2$ $43.2 \times 10^{-5}$ $3 \times 10^{-2}$ $1 \times 10^{-3}$ $3$ $86.4 \times 10^{-5}$ $3 \times 10^{-2}$ $2 \times 10^{-3}$
| Expt | $\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$ | $[NO] \ (mol \ L^{-1})$ | $[H_2] \ (mol \ L^{-1})$ |
| $1$ | $4.8 \times 10^{-5}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
| $2$ | $43.2 \times 10^{-5}$ | $3 \times 10^{-2}$ | $1 \times 10^{-3}$ |
| $3$ | $86.4 \times 10^{-5}$ | $3 \times 10^{-2}$ | $2 \times 10^{-3}$ |
The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:
Exp. $[A] \ (mol \ L^{-1})$ $[B_2] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ S^{-1})$ $1$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $2$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $3$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
Determine the rate law for the reaction.
| Exp. | $[A] \ (mol \ L^{-1})$ | $[B_2] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ S^{-1})$ |
|---|---|---|---|
| $1$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
Determine the rate law for the reaction.
Difficult
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