The decomposition of substance $A$ follows first-order kinetics. Flask $I$ contains $1 \ L$ of $1 \ M$ solution of $A$,and flask $II$ contains $100 \ mL$ of $0.6 \ M$ solution of $A$. After $8 \ hours$,the concentration of $A$ in flask $I$ becomes $0.25 \ M$. How many hours will it take for the concentration of $A$ in flask $II$ to become $0.3 \ M$?
- A$0.4$
- B$2.4$
- C$4.0$
- DCannot be determined as the rate constant is not given.
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Which of the following relations is correct for the given reaction orders?
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View SolutionFor the thermal decomposition of $N_2O_{5(g)}$ at constant volume,the following table can be formed for the reaction mentioned below:
$2N_2O_{5(g)} \rightarrow 2N_2O_{4(g)} + O_{2(g)}$
$S.NO$ $Time/s$ Total pressure $(atm)$ $1.$ $0$ $0.6$ $2.$ $100$ $X$
$X = . . . . . . \times 10^{-3} \ atm$ [nearest integer]
Given: Rate constant for the reaction is $4.606 \times 10^{-2} \ s^{-1}$.
$2N_2O_{5(g)} \rightarrow 2N_2O_{4(g)} + O_{2(g)}$
| $S.NO$ | $Time/s$ | Total pressure $(atm)$ |
| $1.$ | $0$ | $0.6$ |
| $2.$ | $100$ | $X$ |
$X = . . . . . . \times 10^{-3} \ atm$ [nearest integer]
Given: Rate constant for the reaction is $4.606 \times 10^{-2} \ s^{-1}$.
DifficultJEE MAIN 2025
View Solution$A$ first order reaction is $75\%$ completed in $100 \ min$. How long will it take for its $87.5\%$ completion? (in $\min$)
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View SolutionThe first order reaction $A_{(g)} \rightarrow B_{(g)} + 2C_{(g)}$ occurs at $25^{\circ} C$. After $24 \ min$,the ratio of the concentration of products to the concentration of the reactant is $1:3$. What is the half-life of the reaction (in $min$)? $(\log 1.11 = 0.046)$
Which of the following is a first order reaction?
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