For the reaction $2 N_2O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$,the initial concentration of $N_2O_5$ is $2.0 \ mol \ L^{-1}$ and after $300 \ min$,it is reduced to $1.4 \ mol \ L^{-1}$. The rate of production of $NO_2$ (in $mol \ L^{-1} \ min^{-1}$) is
- A$2.5 \times 10^{-4}$
- B$4 \times 10^{-4}$
- C$2.5 \times 10^{-3}$
- D$4 \times 10^{-3}$
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What is chemical kinetics? Which information is obtained by chemical kinetics and thermodynamics regarding a reaction?
Easy
View SolutionFor the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$
Medium
View Solution$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:
The concentration of a reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $10 \ \text{minutes}$. The rate of the reaction is
Easy
View SolutionConsider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:
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