Medium
The 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 | $\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$ | $[NO] \ (mol \ L^{-1})$ | $[H_2] \ (mol \ L^{-1})$ |
| $1$ | $4.8 \times 10^{-5}$ | $1 \times 10^{-2}$ | $1 \times 10^{-3}$ |
| $2$ | $43.2 \times 10^{-5}$ | $3 \times 10^{-2}$ | $1 \times 10^{-3}$ |
| $3$ | $86.4 \times 10^{-5}$ | $3 \times 10^{-2}$ | $2 \times 10^{-3}$ |
- A$\frac{-d[NO]}{dt} = k[NO]^2[H_2]$
- B$\frac{-d[NO]}{dt} = k[NO]^2[H_2]^{\frac{1}{2}}$
- C$\frac{-d[NO]}{dt} = k[NO][H_2]^2$
- D$\frac{-d[NO]}{dt} = k[NO][H_2]$
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For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?
Medium
View SolutionFor the reaction $A_2 + B_2 \to 2AB$,the experimental data is given below. Determine the order of the reaction.
Experiment No. $[A_2] \text{ (M)}$ $[B_2] \text{ (M)}$ Rate $(M \cdot s^{-1})$ $1$ $0.1$ $0.1$ $1.6 \times 10^{-4}$ $2$ $0.1$ $0.2$ $3.2 \times 10^{-4}$ $3$ $0.2$ $0.1$ $3.2 \times 10^{-4}$
| Experiment No. | $[A_2] \text{ (M)}$ | $[B_2] \text{ (M)}$ | Rate $(M \cdot s^{-1})$ |
| $1$ | $0.1$ | $0.1$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.1$ | $0.2$ | $3.2 \times 10^{-4}$ |
| $3$ | $0.2$ | $0.1$ | $3.2 \times 10^{-4}$ |
Medium
View SolutionDuring the kinetic study of the reaction $2A + B \rightarrow C + D$,the following results were obtained:
Experiment $[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$ $i. \ [A]=0.1, [B]=0.1$ $6.0 \times 10^{-3} \ M \ s^{-1}$ $ii. \ [A]=0.3, [B]=0.2$ $7.2 \times 10^{-2} \ M \ s^{-1}$ $iii. \ [A]=0.3, [B]=0.4$ $2.88 \times 10^{-1} \ M \ s^{-1}$ $iv. \ [A]=0.4, [B]=0.1$ $2.40 \times 10^{-2} \ M \ s^{-1}$
Based on the above data,the overall order of the reaction is:
| Experiment | $[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$ |
|---|---|
| $i. \ [A]=0.1, [B]=0.1$ | $6.0 \times 10^{-3} \ M \ s^{-1}$ |
| $ii. \ [A]=0.3, [B]=0.2$ | $7.2 \times 10^{-2} \ M \ s^{-1}$ |
| $iii. \ [A]=0.3, [B]=0.4$ | $2.88 \times 10^{-1} \ M \ s^{-1}$ |
| $iv. \ [A]=0.4, [B]=0.1$ | $2.40 \times 10^{-2} \ M \ s^{-1}$ |
Based on the above data,the overall order of the reaction is:
For the non-stoichiometric reaction $2A + B \to C + D$,the following kinetic data were obtained in three separate experiments,all at $298 \ K$.
Initial Conc. $(A)$ Initial Conc. $(B)$ Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ $0.1 \ M$ $0.1 \ M$ $1.2 \times 10^{-3}$ $0.1 \ M$ $0.2 \ M$ $1.2 \times 10^{-3}$ $0.2 \ M$ $0.1 \ M$ $2.4 \times 10^{-3}$
For the reaction,the rate of formation of $C$ will be:
| Initial Conc. $(A)$ | Initial Conc. $(B)$ | Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $1.2 \times 10^{-3}$ |
| $0.1 \ M$ | $0.2 \ M$ | $1.2 \times 10^{-3}$ |
| $0.2 \ M$ | $0.1 \ M$ | $2.4 \times 10^{-3}$ |
For the reaction,the rate of formation of $C$ will be:
Medium
View SolutionThe unit of the rate constant depends on which of the following?
Easy
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