Chemical Kinetics

The rate constants for decomposition of acetaldehyde have been measured over the temperature range 700 - 1000 K. The data has been analysed by plotting $\ln k$ vs $\dfrac{10^3}T$ graph. The value of activation energy for the reaction is ______ $\mathrm{kJ\,mol^{-1}}$. (Nearest integer)

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

For a first order reaction, the time required for completion of 90% reaction is 'x' times the half life of the reaction. The value of 'x' is

(Given: $\ln10=2.303$ and $\log2=0.3010$)

For a given chemical reaction
$$\gamma_1A+\gamma_2B\rightarrow\gamma_3C+\gamma_4D$$
Concentration of C changes from 10 mmol dm$^{-3}$ to 20 mmol dm$^{-3}$ in 10 seconds. Rate of appearance of D is 1.5 times the rate of disappearance of B which is twice the rate of disappearance A. The rate of appearance of D has been experimentally determined to be 9 mmol dm$^{-3}$ s$^{-1}$. Therefore the rate of reaction is ______ mmol dm$^{-3}$ s$^{-1}$. (Nearest Integer)

At 345 K, the half life for the decomposition of a sample of a gaseous compound initially at 55.5 kPa was 340 s. When the pressure was 27.8 kPa, the half life was found to be 170 s. The order of the reaction is ______. [integer answer]

A flask is filled with equal moles of A and B. The half lives of A and B are 100 s and 50 s respectively and are independent of the initial concentration. The time required for the concentration of A to be four times that of B is ______ s.

(Given : $\ln2=0.693$)

Catalyst A reduces the activation energy for a reaction by 10 kJ mol$^{-1}$ at 300 K. The ratio of rate constants, $\dfrac{k_{T,\text{Catalysed}}}{k_{T,\text{Uncatalysed}}}$ is $e^x$. The value of $x$ is ______. [nearest integer]

[Assume that the pre-exponential factor is same in both the cases. Given $R=8.31$ J K$^{-1}$mol$^{-1}$]

The rate constant for a first order reaction is given by the following equation :
$$\ln k=33.24-\frac{2.0\times10^4\ \mathrm K}T$$
The Activation energy for the reaction is given by ______ kJ mol$^{-1}$. (In Nearest integer)

(Given : $R=8.3$ J K$^{-1}$ mol$^{-1}$)

It has been found that for a chemical reaction with rise in temperature by 9 K the rate constant gets doubled. Assuming a reaction to be occurring at 300 K, the value of activation energy is found to be ______ kJ mol$^{-1}$. [nearest integer]

(Given $\ln10=2.3$, $R=8.3$ J K$^{-1}$ mol$^{-1}$, $\log2=0.30$)

For a first order reaction A $\rightarrow$ B, the rate constant, k = $5.5\times10^{-14}$ s$^{-1}$. The time required for 67% completion of reaction is $x\times10^{-1}$ times the half life of reaction. The value of $x$ is ______ (Nearest integer)

(Given : log 3 = 0.4771)

A radioactive element has a half life of 200 days. The percentage of original activity remaining after 83 days is ______. (Nearest integer)

(Given : antilog 0.125 = 1.333, antilog 0.693 = 4.93)

The activation energy of one of the reactions in a biochemical process is 532611 J mol$^{-1}$. When the temperature falls from 310 K to 300 K, the change in rate constant observed is $k_{300}=x\times10^{-3}k_{310}$. The value of $x$ is ______.

[Given : ln10 = 2.3; R = 8.3 J K$^{-1}$ mol$^{-1}$]

The equation $k=\left(6.5\times10^{12}\text{s}^{-1}\right)e^{-26000\text{K}/T}$ is followed for the decomposition of compound A. The activation energy for the reaction is ______ kJ mol$^{-1}$. [nearest integer]

(Given: R = 8.314 J K$^{-1}$mol$^{-1}$)

For the reaction P → B, the values of frequency factor A and activation energy $E_A$ are $4\times10^{13}$ s$^{-1}$ and 8.3 kJ mol$^{-1}$ respectively. If the reaction is of first order, the temperature at which the rate constant is $2\times10^{-6}$ s$^{-1}$ is ______ $\times10^{-1}$ K

(Given : ln 10 = 2.3, R = 8.3 J K$^{-1}$ mol$^{-1}$, log2 = 0.30)

The half life for the decomposition of gaseous compound A is 240 s when the gaseous pressure was 500 Torr initially. When the pressure was 250 Torr, the half life was found to be 4.0 min. The order of the reaction is ______. (Nearest integer)

For the decomposition of azomethane, $\mathrm{CH_3N_2CH_3(g)\rightarrow CH_3CH_3(g)+N_2(g)}$, a first order reaction, the variation in partial pressure with time at 600 K is given as

The half life of the reaction is ______ $\times10^{-5}$ s. [Nearest integer]

For a reaction A → 2B + C the half lives are 100 s and 50 s when the concentration of reactant A is 0.5 and 1.0 mol L$^{-1}$ respectively. The order of the reaction is ______. (Nearest Integer)

At 30°C, the half life for the decomposition of $\mathrm{AB_2}$ is 200 s and is independent of the initial concentration of $\mathrm{AB_2}$. The time required for 80% of the $\mathrm{AB_2}$ to decompose is

Given: log 2 = 0.30, log 3 = 0.48

$$\mathrm{2NO+2H_2\rightarrow N_2+2H_2O}$$

The above reaction has been studied at 800°C. The related data are given in the table below

Reaction serial number	Initial Pressure of $\mathrm{H_2}$ / kPa	Initial Pressure of NO / kPa	Initial rate $\left(\dfrac{-dp}{dt}\right)$ / (kPa/s)
1	65.6	40.0	0.135
2	65.6	20.1	0.033
3	38.6	65.6	0.214
4	19.2	65.6	0.106

The order of the reaction with respect to NO is ______.

$$\underset{\text{Reactant}}{[A]}\rightarrow\underset{\text{Product}}{[B]}$$

If formation of compound [B] follows the first order of kinetics and after 70 minutes the concentration of [A] was found to be half of its initial concentration. Then the rate constant of the reaction is $x\times10^{-6}$ s$^{-1}$. The value of $x$ is ______. (Nearest Integer)

For kinetic study of the reaction of iodide ion with $\mathrm{H_2O_2}$ at room temperature :

(A) Always use freshly prepared starch solution.
(B) Always keep the concentration of sodium thiosulphate solution less than that of KI solution.
(C) Record the time immediately after the appearance of blue colour.
(D) Record the time immediately before the appearance of blue colour.
(E) Always keep the concentration of sodium thiosulphate solution more than that of KI solution.

Choose the correct answer from the options given below :