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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In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is:
For the reaction $2N_2O_5(g) \rightleftharpoons 4NO_2(g) + O_2(g)$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \ mol \ L^{-1}$ in $5 \ s$. Calculate the rate of change of concentration of $N_2O_5$.
Medium
View Solution$N_2 + 3H_2 \to 2NH_3$. If the concentration of $NH_3$ changes from $0.01 \ M$ to $0.04 \ M$ in $20 \ seconds$,then the rate of reaction will be:
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Difficult
View SolutionIdentify the correct expression for the rate of the following reaction: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
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