For the reaction system $2NO_{(g)} + O_{2(g)} \to 2NO_{2(g)}$,the volume is suddenly reduced to half its initial value by increasing the pressure. If the reaction is of first order with respect to $O_2$ and second order with respect to $NO$,the rate of reaction will:
- ADiminish to one fourth of its initial value
- BDiminish to one eighth of its initial value
- CIncrease to eight times of its initial value
- DIncrease to four times of its initial value
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An example of a pseudo-$unimolecular$ reaction is
Easy
View SolutionThe following are the rate constants of two different reactions. Determine the overall order of reaction for each case:
$(a)$ $6.66 \times 10^{-3} \, s^{-1}$
$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$
$(a)$ $6.66 \times 10^{-3} \, s^{-1}$
$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$
Medium
View SolutionWhat is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
Difficult
View SolutionAn elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?
Medium
View SolutionWrite the unit of the rate constant for the following reactions:
$1.$ $5/2$ order
$2.$ $n$ order
$1.$ $5/2$ order
$2.$ $n$ order
Easy
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