Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?
- AConcentration of $A$ is doubled and concentration of $B$ is kept constant.
- BConcentration of $B$ is doubled and concentration of $A$ is kept constant.
- CConcentration of $B$ is doubled and concentration of $A$ is halved.
- DConcentration of $A$ is kept constant and concentration of $B$ is halved.
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$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
$Run$ $[NO]_{0}$ $[Cl_{2}]_{0}$ $r_{0}$ $1$ $0.10$ $0.10$ $0.18$ $2$ $0.10$ $0.20$ $0.35$ $3$ $0.20$ $0.20$ $1.40$
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
| $Run$ | $[NO]_{0}$ | $[Cl_{2}]_{0}$ | $r_{0}$ |
| $1$ | $0.10$ | $0.10$ | $0.18$ |
| $2$ | $0.10$ | $0.20$ | $0.35$ |
| $3$ | $0.20$ | $0.20$ | $1.40$ |
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
For the reaction,$PCl_5 \longrightarrow PCl_3 + Cl_2$,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 at a given instant. The molar concentration of $PCl_5$ at that instant is
MediumKCET 2024
View SolutionThe order of a reaction with rate equals $k[C_A]^{3/2} [C_B]^{-1/2}$ is
Medium
View SolutionThe half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$ $t_{1/2} \text{ (minutes)}$ $135$ $112.5$
The order of reaction is -
| $P_0 \text{ (mmHg)}$ | $250$ | $300$ |
| $t_{1/2} \text{ (minutes)}$ | $135$ | $112.5$ |
The order of reaction is -
Medium
View SolutionFor the reaction: $2 A + B \rightarrow A_2 B$,the rate $= k[A][B]^2$ with $k = 2.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$. Calculate the initial rate of the reaction when $[A] = 0.1 \ mol \ L^{-1}$ and $[B] = 0.2 \ mol \ L^{-1}$. Calculate the rate of reaction after $[A]$ is reduced to $0.06 \ mol \ L^{-1}$.
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