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$4 \times 10^{-3}$
Explore More
Similar Questions
In the reaction $2 N_{2}O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the ratio of the rate of formation of $NO_{2(g)}$ to the rate of formation of $O_{2(g)}$ is:
Find the rate of formation of $NO_{2(g)}$ in the following reaction.
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$
$A$ reaction,$3 X_{(g)} \rightarrow 2 Y_{(g)} + Z_{(g)}$ takes place in a closed vessel. What is the rate of formation of $Y$ (in $mol \ L^{-1} \ s^{-1}$) if the rate of disappearance of $X$ is $7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$?
Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.
Easy
View SolutionFor the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ h^{-1}$. The rate of conversion of $H_2$ under the same conditions is:
MediumIIT 1994
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo