To determine the activation energy of the reaction using the Arrhenius equation, the student should follow these steps:1. Collect data: The student should perform the reaction at least two different temperatures T1 and T2 and measure the corresponding reaction rates k1 and k2 .2. Understand the Arrhenius equation: The Arrhenius equation is given by k = A * exp -Ea / R * T , where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant 8.314 J/mol*K , and T is the temperature in Kelvin.3. Take the natural logarithm of the Arrhenius equation: ln k = ln A - Ea / R * T .4. Calculate the natural logarithm of the rate constants: Calculate ln k1 and ln k2 using the measured reaction rates.5. Set up two equations using the Arrhenius equation for both temperatures: ln k1 = ln A - Ea / R * T1 and ln k2 = ln A - Ea / R * T2 .6. Subtract the two equations to eliminate the pre-exponential factor A : ln k2/k1 = Ea / R * 1/T1 - 1/T2 .7. Rearrange the equation to solve for Ea: Ea = R * ln k2/k1 / 1/T1 - 1/T2 .8. Plug in the values: Substitute the values of R, k1, k2, T1, and T2 into the equation and solve for Ea.9. Calculate the activation energy: The result will be the activation energy of the reaction in units of Joules per mole J/mol .By following these steps, the student can determine the activation energy of the reaction between hydrogen and chlorine gases using the Arrhenius equation.