Prof. Anil Thomas and Prof. Santosh Yadav Solutions for Chapter: Chemical Kinetics, Exercise 4: Evaluation Test

The initial rates of reaction $3\mathrm{A}+2\mathrm{B}+\mathrm{C}\stackrel{}{\to }$Products, at different initial concentrations are given below:

The order with respect to the reactants, $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$, respectively is:

The rate law for the reaction Sucrose $+$ Water $\stackrel{{\text{[H}}^{\text{+}}\text{]}}{\to }$ Glucose $+$ Fructose is given by:

The rates of a certain reaction $(\mathrm{dc}/\mathrm{dt})$ at different times are as follows:

The reaction is:

The rate law for a reaction between the substances $\mathrm{A}$ and $\mathrm{B}$ is given by, rate$=$ $\mathrm{k} [\mathrm{A}{]}^{\mathrm{n}} [\mathrm{B}{]}^{\mathrm{m}}$. On doubling the concentration of $\mathrm{A}$ and halving the concentration of $\mathrm{B}$, the ratio of the new rate to the earlier rate of the reaction will be:

An exothermic reaction A $\stackrel{}{\to }$B has activation energy of $17 \mathrm{kJ}$ per mole of A. The heat of the reaction is 40 kJ. Calculate the activation energy for the reverse reaction B $\stackrel{}{\to }$A

Which of the following stands TRUE for molecularity of a reaction?

Which is the INCORRECT statement about rate of reaction?

For the reaction ${\mathrm{N}}_{2 \left(\mathrm{g}\right)} + 3{\mathrm{H}}_{2 \left(\mathrm{g}\right)}\stackrel{}{\to } 2{\mathrm{NH}}_{3 \left(\mathrm{g}\right),}$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of ${\mathrm{NH}}_{\mathrm{3}}\text{ is} 0.001 \mathrm{kg} {\mathrm{hr}}^{-1}$. The rate of conversion of ${\mathrm{H}}_{\mathrm{2}}$ under the same conditions is: