Medium
The half-life period of a $second$ order reaction is:
- AProportional to the initial concentration of reactants
- BIndependent of the initial concentration of reactants
- CInversely proportional to the initial concentration of reactants
- DInversely proportional to the square of the initial concentration of reactants
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Similar Questions
Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$
$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$
| $Expt. \ No.$ | $[A]$ | $[B]$ | $Initial \ Rate$ |
|---|---|---|---|
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.070$ | $0.80$ |
| $3$ | $0.024$ | $0.035$ | $0.10$ |
| $4$ | $0.012$ | $0.070$ | $0.80$ |
DifficultAIIMS 2015
View SolutionFrom the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(iii)$ $CH_{3}CHO_{(g)} \rightarrow CH_{4(g)} + CO_{(g)} \quad$ Rate $= k[CH_{3}CHO]^{3/2}$
$(iii)$ $CH_{3}CHO_{(g)} \rightarrow CH_{4(g)} + CO_{(g)} \quad$ Rate $= k[CH_{3}CHO]^{3/2}$
Medium
View SolutionFor the reaction: $2A + B \to A_2B$; the rate $= K[A][B]^2$ with $K = 2.0 \times 10^{-6} \ L^2 \ mol^{-2} \ s^{-1}$. Initial concentrations of $A$ and $B$ are $[A]_0 = 0.2 \ mol/L$ and $[B]_0 = 0.4 \ mol/L$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12 \ mol/L$.
Medium
View SolutionFor the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?
Certain bimolecular reactions which follow the first order kinetics are called
Easy
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