Which of the following equations is correct regarding the rate of disappearance of reactant and appearance of product for the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$?
- A$-\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt}$
- B$-\frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$
- C$\frac{d[NH_3]}{dt} = \frac{1}{3} \frac{d[H_2]}{dt}$
- D$3 \frac{d[NH_3]}{dt} = -2 \frac{d[H_2]}{dt}$
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Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?
$NO_2$ required for a reaction is produced by the decomposition of $N_2O_5$ in $CCl_4$ as per the equation $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$. The initial concentration of $N_2O_5$ is $3.00 \, mol \, L^{-1}$ and it is $2.75 \, mol \, L^{-1}$ after $30 \, minutes$. The rate of formation of $NO_2$ is ............... $mol \, L^{-1} \, min^{-1}$
DifficultJEE MAIN 2019
View SolutionFind the rate of formation of $NO_{2(g)}$ in the following reaction.
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
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For a chemical reaction $4 A + 3 B \rightarrow 6 C + 9 D$,the rate of formation of $C$ is $6 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$ and the rate of disappearance of $A$ is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction and the amount of $B$ consumed in an interval of $10 \ s$,respectively,will be:
MediumNEET 2022
View SolutionFor the reaction $3 A + 2 B \rightarrow C$,which statement is correct $:-$
Medium
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