For 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:
- A$1.82 \times 10^{-4} \ kg \ h^{-1}$
- B$0.0015 \ kg \ h^{-1}$
- C$1.52 \times 10^{4} \ kg \ h^{-1}$
- D$1.82 \times 10^{-14} \ kg \ h^{-1}$
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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
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$(i)$ Rate of Reaction
$(ii)$ Average rate of reaction
$(iii)$ Instantaneous rate
$(i)$ Rate of Reaction
$(ii)$ Average rate of reaction
$(iii)$ Instantaneous rate
Difficult
View SolutionWhich one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?
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