Chemical Kinetics · Chemistry · NEET

$$ \text { Match List I with List II : } $$

For a certain reaction $R \rightarrow$ Product, the plot of concentration $[R]$ vs time has a negative slope as shown. The order of reaction is :

Given below is an expression for the rate constant of a first-order reaction occurring at a certain temperature, $\mathrm{T}(\mathrm{K})$.

$$ \operatorname{lnk}=14.34-\frac{1.25 \times 10^4}{T} $$

The energy of activation in $\mathrm{kcal} \mathrm{mol}^{-1}$ for the reaction is :

(Given: $\mathrm{k}^{-1} \mathrm{~s} \mathrm{~s}^{-1}, \mathrm{R}=1.987 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$ )

If the rate constant of a reaction is $0.03 \mathrm{~s}^{-1}$, how much time does it take for $7.2 \mathrm{~mol} \mathrm{~L}^{-1}$ concentration of the reactant to get reduced to $0.9 \mathrm{~mol} \mathrm{~L}^{-1}$ ? (Given: $\log 2=0.301$ )

If the half-life ( $t_{1 / 2}$ ) for a first order reaction is 1 minute, then the time required for $99.9 \%$ completion of the reaction is closest to :

Following data is for a reaction between reactants A and B :

$$ \text { The order of the reaction with respect to } \mathrm{A} \text { and } \mathrm{B} \text {, respectively, are } $$

Which of the following plot represents the variation of $$\ln \mathrm{k}$$ versus $$\frac{1}{\mathrm{~T}}$$ in accordance with Arrhenius equation?

Rate constants of a reaction at $$500 \mathrm{~K}$$ and $$700 \mathrm{~K}$$ are $$0.04 \mathrm{~s}^{-1}$$ and $$0.14 \mathrm{~s}^{-1}$$, respectively; then, activation energy of the reaction is :

(Given: $$\log 3.5=0.5441, \mathrm{R}=8.31 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$$)

Activation energy of any chemical reaction can be calculated if one knows the value of

Which plot of $$\ln \mathrm{k}$$ vs $$\frac{1}{\mathrm{~T}}$$ is consistent with Arrhenius equation?

The rate of a reaction quadruples when temperature changes from $$27^{\circ} \mathrm{C}$$ to $$57^{\circ} \mathrm{C}$$. Calculate the energy of activation.

Given $$\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6021$$

For a reaction $$3 \mathrm{~A} \rightarrow 2 \mathrm{~B}$$

The average rate of appearance of $$\mathrm{B}$$ is given by $$\frac{\Delta[B]}{\Delta t}$$. The correct relation between the average rate of appearance of $$\mathrm{B}$$ with the average rate of disappearance of A is given in option :

The correct options for the rate law that corresponds to overall first order reaction is

For a certain reaction, the rate $$=\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}]$$, when the initial concentration of A is tripled keeping concentration of $$\mathrm{B}$$ constant, the initial rate would

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A : A reaction can have zero activation energy.

Reason R : The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

In the light of the above statements, choose the correct answer from the options given below:

For a chemical reaction

4A + 3B $$\to$$ 6C + 9D

Rate of formation of C is 6 $$\times$$ 10^$$-$$2 mol L^$$-$$1 s^$$-$$1 and rate of disappearance of A is 4 $$\times$$ 10^$$-$$2 mol L^$$-$$1 s^$$-$$1. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be :

The given graph is a representation of kinetics of a reaction

The y and x axes for zero and first order reactions, respectively are

For a first order reaction A $$\to$$ Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min^$$-$$1 is