Chemical Kinetics Test

The rate constant of the reaction at temperature 200 K is 10 times less than the rate constant at 400 K. The activation energy of the reaction is

The slope in the log k vs. 1/T curve is $5.42{\text{ }} \times {\text{ }}{10^3}$. The value of the activation energy is approximately

The half life periods of a reaction at initial concentration 0.1 mol/L and 0.5 mol/L are 200 s and 40 s respectively. The order of the reaction is

The half life of a substance in a first order reaction is 15 min. The rate constant is

The reaction $2A \to B$is first order in A with a rate constant of 2.8 X10$ ^{– 2}$$s^{ – 1}$. How long will it take for A to decrease from 0.88 M to 0.14 M?

When 10 g of radioactive isotope is reduced to 1.25 g in 12 years, the half life period of the isotope is

The value of decay constant of a compound having a half life period of 2.95 days is

The reaction $2{\text{ }}NO{\text{ }} + {\text{ }}B{r_2} \to 2NOBr$ follows the mechanism given belowIf the concentration of both NO and Br2 are increased two times, the rate of reaction would become

$E_a$ for the reaction is 1.18 X 10$^5$ J/mol. The slope of the graph of log k vs. 1/T is

For the reaction A$ \to $ products, at$\left[ A \right]{\text{ }} = {\text{ }}0.4{\text{ }}M,{\text{ }}{t_{1/2}} = 24{\text{ }}s$ and at $\left[ A \right]{\text{ }} = {\text{ }}0.2{\text{ }}M,{\text{ }}{t_{1/2}} = {\text{ }}12{\text{ }}s$. The unit for the rate constant is

For the reaction ${\text{A }} \rightleftarrows {\text{ B, \Delta H = + 40 kJ/mol}}{\text{. If }}{{\text{E}}_{\text{a}}}$for the backward reaction is 60 kJ/mol. $E_a$ for the forward reaction is

For the reaction A + 3B $ \to $2C + 2D, the concentration of A changes from 0.150 M to 0.0135 M in 1 min. The rate of formation of C in mol/L/s is

Thermal decomposition of a compound is of first order. If 50% of a sample of a compound is decomposed in 120 min, the time taken for 99.9%completion is

In the catalyzed decomposition of benzene diazonium chloride, Half life period is found to be independent of the initial concentration of the reactant. After 10 min, the volume of $N_2$ gas collected is 10 L and after the reaction is complete, it is 50 L. Hence, the rate constant of the reaction(in min $^{– 1}$) is

Decomposition of$ H_2O_24$ was studied by titration against $KMnO_4$ solution. It was found that 0.4 mol of H2O2 was reduced to 0.2 mol in 20 min and to 0.1 mol in 40 min and to 0.05 mol after 1 hr. the order of reaction must be