For the chemical reaction $N_{2(g)} + 3 H_{2(g)} \rightleftharpoons 2 NH_{3(g)}$,the correct option is
- A$-\frac{1}{3} \frac{d[H_{2}]}{dt} = -\frac{1}{2} \frac{d[NH_{3}]}{dt}$
- B$-\frac{d[N_{2}]}{dt} = 2 \frac{d[NH_{3}]}{dt}$
- C$-\frac{d[N_{2}]}{dt} = \frac{1}{2} \frac{d[NH_{3}]}{dt}$
- D$3 \frac{d[H_{2}]}{dt} = 2 \frac{d[NH_{3}]}{dt}$
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Similar Questions
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 $mol \ L^{-1} \ min^{-1}$)?
$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?
Difficult
View SolutionIn the hydrolysis reaction of butyl chloride,the concentration of reactant at $600 \ s$ is determined using a tangent at $t_2 = 800 \ s$ and $t_1 = 400 \ s$. Given the concentrations $[R_2] = 0.0165 \ mol \ L^{-1}$ and $[R_1] = 0.037 \ mol \ L^{-1}$,calculate the instantaneous rate $r_{ins}$ at $600 \ s$.
Medium
View SolutionFor the reaction $3 \,A \rightarrow 2 \,B$, the rate of reaction $+\frac{d[B]}{d t}$ is equal to:
Explain how the rate of reaction depends on concentration and time using graphs.
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