Final answer:
The activation energy can be calculated using the rate constant and the slope of the linear plot.
Step-by-step explanation:
The activation energy for a chemical reaction can be determined by measuring the effect of temperature on the reaction rate. In this case, the natural logarithm of the reaction rate constant is plotted against the reciprocal of the temperature in Kelvin degrees. The resulting linear plot has a slope of the rate constant (k) and a y-intercept of 26.3.
To calculate the activation energy, we can use the equation:
k = Ae^(-Ea/RT)
Where k is the reaction rate constant, A is the frequency factor (also known as pre-exponential factor), Ea is the activation energy, R is the universal gas constant (8.314 J/Kmol), and T is the temperature in Kelvin.
By rearranging the equation, we can isolate Ea:
Ea = -slope * R
In this case, the slope of the linear plot is the rate constant (k), so Ea = -26.3 * 8.314 J/Kmol.
Substituting the values, we can calculate the activation energy.