Slope of the graph given is \(-9.2 J/mol\). The activation energy of the reaction is :

\(76.48\, \ J/mol\)

The correct answer is option 1. \(76.48\, \ J/mol\).

The given graph is:

Given that the slope of the graph is \(-9.2 \, \text{J/mol}\), we can determine the activation energy (\(E_a\)) using the Arrhenius equation:

\(\text{Slope} = -\frac{E_a}{R}\)

where:

The slope is given as \(-9.2 \, \text{J/mol}\).

\(R\) is the gas constant, \(8.314 \, \text{J/mol·K}\).

Rearranging to solve for \(E_a\):

\(-9.2 = -\frac{E_a}{8.314}\)

\(E_a = 9.2 \times 8.314\)

\(E_a = 76.48 \, \text{J/mol}\)

So, the activation energy of the reaction is: 1. \(76.48 \, \text{J/mol}\)