Medium
The rate law for the reaction $A + B \rightarrow \text{product}$ is given by $\text{rate} = k[A][B]$. Calculate $[A]$ if the rate of reaction and rate constant are $0.25 \ mol \ dm^{-3} \ s^{-1}$ and $6.25 \ mol^{-1} \ dm^3 \ s^{-1}$ respectively,and $[B] = 0.25 \ mol \ dm^{-3}$.
- A$0.22 \ mol \ dm^{-3}$
- B$0.16 \ mol \ dm^{-3}$
- C$0.30 \ mol \ dm^{-3}$
- D$0.25 \ mol \ dm^{-3}$
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View SolutionThe following results are obtained for the reaction $S + Nu \rightarrow \text{product}$. By which reaction mechanism does this reaction occur?
Experiment $[S]$ $[Nu]$ Rate $1$ $0.1$ $0.1$ $2.2 \times 10^{-3}$ $2$ $0.2$ $0.1$ $4.4 \times 10^{-3}$ $3$ $0.1$ $0.2$ $4.4 \times 10^{-3}$
| Experiment | $[S]$ | $[Nu]$ | Rate |
|---|---|---|---|
| $1$ | $0.1$ | $0.1$ | $2.2 \times 10^{-3}$ |
| $2$ | $0.2$ | $0.1$ | $4.4 \times 10^{-3}$ |
| $3$ | $0.1$ | $0.2$ | $4.4 \times 10^{-3}$ |
The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.
MediumAIIMS 2011
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