$R \longrightarrow P$ is a first order reaction. The concentration of $R$ changed from $0.04$ to $0.03 \ mol \ L^{-1}$ in $40 \ min$. What is the average velocity of the reaction in $mol \ L^{-1} \ s^{-1}$?
- A$2.5 \times 10^{-4}$
- B$4.167 \times 10^{-6}$
- C$4.167 \times 10^{6}$
- D$2.5 \times 10^{-5}$
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For the reaction $2N_2O_5(g) \rightleftharpoons 4NO_2(g) + O_2(g)$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \ mol \ L^{-1}$ in $5 \ s$. Calculate the rate of change of concentration of $N_2O_5$.
Medium
View SolutionFor the reaction $2A \rightarrow 3C + D$, the rate of reaction is represented by:
For the reaction,$A + 3B \longrightarrow 2C$,the rate of consumption of $A$ is $1.4 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of formation of $C$.
From the concentrations of $C_{4}H_{9}Cl$ (butyl chloride) at different times given below,calculate the average rate of the reaction:
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
$t/s$ $0$ $50$ $100$ $150$ $200$ $300$ $400$ $700$ $800$ $[C_{4}H_{9}Cl]/mol\ L^{-1}$ $0.100$ $0.0905$ $0.0820$ $0.0741$ $0.0671$ $0.0549$ $0.0439$ $0.0210$ $0.017$
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
| $t/s$ | $0$ | $50$ | $100$ | $150$ | $200$ | $300$ | $400$ | $700$ | $800$ |
| $[C_{4}H_{9}Cl]/mol\ L^{-1}$ | $0.100$ | $0.0905$ | $0.0820$ | $0.0741$ | $0.0671$ | $0.0549$ | $0.0439$ | $0.0210$ | $0.017$ |
Difficult
View SolutionFor the chemical reaction $N_{2(g)} + 3 H_{2(g)} \rightleftharpoons 2 NH_{3(g)}$,the correct option is
DifficultNEET 2019
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