For a first-order reaction,the rate constant is $60 \ s^{-1}$. How much time will it take for the initial concentration of the reactant to be reduced to $1/10$th of its initial value?
- A$3.8 \times 10^{-2} \ s$
- B$1.26 \times 10^{13} \ s$
- C$2.01 \times 10^{13} \ s$
- D$1.097 \times 10^{13} \ s$
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$A$ first-order reaction is $50\%$ complete in $45 \text{ minutes}$. How many hours will it take for the reaction to be $99.9\%$ complete?
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View Solution$A_{(g)} \rightarrow B_{(g)} + C_{(g)}$ is a first order reaction.
Time $t$ $\infty$ $P_{\text{system}}$ $P_t$ $P_{\infty}$
The reaction was started with reactant $A$ only. Which of the following expressions is correct for the rate constant $k$?
| Time | $t$ | $\infty$ |
| $P_{\text{system}}$ | $P_t$ | $P_{\infty}$ |
The reaction was started with reactant $A$ only. Which of the following expressions is correct for the rate constant $k$?
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The half-life values for two different first-order reactions $A$ and $B$ are $75 \ min$ and $2.5 \ h$ respectively. What is the ratio of their rate constants $\frac{k_A}{k_B}$?
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