Slope of the graph given is \(-9.2 J/mol\). The activation energy of the reaction is :
Answer & explanation
Correct answer: option 1
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. \(76.48 \, \text{J/mol}\)