In \(\frac { { k }_{ 2 } }{ { k }_{ 1 } } =\frac { { E }_{ a } }{ R } \left[ \frac { { T }_{ 2 }-{ T }_{ 1 } }{ { T }_{ 1 }{ T }_{ 2 } } \right] \)
In 2 = \(\frac { { E }_{ a } }{ R } \) \(\left[ \frac { 10 }{ 300\times 310 } \right] \)
E_a = 9300 R In 2
= 53.4 kJ mol^-1

\({ k }=2.303\log { \frac { \left[ { A }_{ 0 } \right] }{ \left[ A \right] } } \)
\(t=\frac { 2.303 }{ { 10 }^{ -3 } } \log { \frac { 10 }{ 2.5 } } \)
t = 2303 x 0.301 x 2 = 1386 s.

(i) Catalyst lowers the activation energy and changes the path of the reaction and thus increases the rate of the reaction. A catalyst does not alter Gibbs energy of a reaction.
(ii) Higher the temperature faster the reaction. This is because increasing the temperature increases the Kinetic energy, and hence more molecules would have energy greater than the activation energy resulting in increased rate and completion of the reaction. Hence oxalic acid should be heated in redox titration against KMnO₄.

(i) The rate of a reaction depends on the concentration of the reactant.
(ii) As the reaction proceeds to forward direction, concentration of reactant decreases and that of product increases.
(iii) So, the rate of reaction generally decreases during the course of reaction.

For n^th reaction
\(K\alpha \frac { 1 }{ { C }^{ n-1 } } \)

Overall order of this reaction = 1+ 2 = 3

Order of the reaction = \(\frac { 1 }{ 2 } +\frac { 3 }{ 2 } =\frac { 4 }{ 2 } =2\)
The reaction is second order.

The order of the reaction is zero.

(i) I Order reaction
(ii) S^-1
(iii) \({ t }_{ \frac { 1 }{ 2 } }\) = 0.693/k

Rate decreases with time as the reaction proceeds and the average rate cannot be used to predict the rate of the reaction at any instant. The rate of the reaction, at a particular instant during the reaction is called the instantaneous rate. So instantaneous rate in prepared over average rate.

The reaction is a zero order reaction whose rate is independent on the concentration of reactants.

Rate of a reaction at any time depends on the concentration of the reactants which keeps on decreasing with time.

Minus sign i.e.  \(\frac { -dA }{ dt } \) or \(\frac { -dB }{ dt } \) indicates decreases in the concentration of reactants whereas + sign indicates in the concentration of products with time i.e. \(\frac { +dC }{ dt } \)

The study of chemical kinetics helps us
(i) To determine the rate of a chemical reaction.
(ii) In optimizing the process conditions of industrial manufacturing processes.