Why does the rate of any reaction generally decrease during the course of the reaction?
(N/A) The rate of a reaction depends on the concentration of reactants. As the reaction progresses,the concentration of reactants decreases because the reactants are converted into products. According to the rate law,the rate is directly proportional to the concentration of reactants. Therefore,as the concentration of reactants decreases,the rate of the reaction also decreases.
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$(a)$ The rate of reaction ....... as the concentration of reactant decreases.
$(b)$ The rate of reaction ....... as the concentration of product increases.
$(a)$ The rate of reaction ....... as the concentration of reactant decreases.
$(b)$ The rate of reaction ....... as the concentration of product increases.
Medium
View SolutionIn a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$
Medium
View SolutionIf the rate of disappearance of $N_2O_5$ in the following reaction is $1.2 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,the rate of production of $NO_2$ in $mol \ L^{-1} \ s^{-1}$ is:
$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$
$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$
For the reaction,$XA + YB \rightarrow ZC$,if $\frac{- d [ A ]}{ dt } = \frac{- d [ B ]}{ dt } = \frac{d [ C ]}{ dt },$ then the correct statement among the following is:
MediumNEET 2017
View SolutionFind the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.
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