Ncert Exercises & Solutions

The activation energy of a chemical reaction can be calculated by:

1.	Determining the rate constant at standard temperature.
2.	Determining the rate constant at two temperatures.
3.	Determining probability of collision.
4.	Using the catalyst.

HINT: The formula used is $In$ $(\frac{k_{1}}{k_{2}})$ $=$ $\frac{E_{a}}{R}$ $[$ $\frac{1}{T_{1}}$ $-$ $\frac{1}{T_{2}}]$

Explanation:

The activation energy of a chemical reaction is related to the rate constant of a reaction at two different temperatures i.e., k₁ and k₂ respectively

$In$ $(\frac{k_{1}}{k_{2}})$ $=$ $\frac{E_{a}}{R}$ $[$ $\frac{1}{T_{1}}$ $-$ $\frac{1}{T_{2}}]$

where,

$\begin{array}{l} E_{a} = activation energy \\ T_{2} = higher temperature \\ T_{1} = lower temperature \\ k_{1} = rate constant at lemperature T_{1} \\ k_{2} = rate constant at temperature T_{2} \end{array}$

This equation is known as the Arrhenius equation.

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