(B) The given rate law is $\text{Rate} = K_1[RCl]$.This indicates that the reaction is of first order with respect to the alkyl halide $(RCl)$ and zer

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Halved on reducing the concentration of alkyl halide to one half

(B) The given rate law is $\text{Rate} = K_1[RCl]$.This indicates that the reaction is of first order with respect to the alkyl halide $(RCl)$ and zero order with respect to sodium hydroxide $(NaOH)$.If the concentration of the alkyl halide is reduced to one half,the new rate will be $\text{Rate}' = K_1 \times \frac{1}{2}[RCl] = \frac{1}{2} \times \text{Rate}$.Therefore,the rate is halved on reducing the concentration of the alkyl halide to one half.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

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The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be

IIT 1988 All IIT

A
Doubled on doubling the concentration of sodium hydroxide
B
Halved on reducing the concentration of alkyl halide to one half
C
Decreased on increasing the temperature of the reaction
D
Unaffected by increasing the temperature of the reaction

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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IIT 1988 Paper All IIT years →

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

MediumIIT 2000

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For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

Difficult

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The three experimental data for determining the differential rate of reaction $2 NO_{(g)} + Cl_{2(g)} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below.
$(a)$ Calculate the order of reaction.
$(b)$ Calculate the value of the rate constant.

Medium

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

Medium

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If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

Medium

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The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

The three experimental data for determining the differential rate of reaction $2 NO_{(g)} + Cl_{2(g)} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below. $(a)$ Calculate the order of reaction.$(b)$ Calculate the value of the rate constant.

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

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The three experimental data for determining the differential rate of reaction $2 NO_{(g)} + Cl_{2(g)} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below.
$(a)$ Calculate the order of reaction.
$(b)$ Calculate the value of the rate constant.

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$