The rate constant k for a certain reaction is measured at two different temperatures:temperature k110.0°C ×4.4105−10.0°C ×1.9102Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy Ea for this reaction.Round your answer to 2 significant digits.

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, and T is the temperature in Kelvin.

We can rearrange the equation to solve for Ea:

Ea = -R * T * ln(k / A)

We have two sets of k and T, so we can set up two equations and solve for Ea. However, we don't know A. But we can eliminate A by dividing one equation by the other:

ln(k1 / k2) = Ea / R * (1/T2 - 1/T1)

We can now plug in the given values and solve for Ea. Remember to convert the temperatures from Celsius to Kelvin (T = °C + 273.15):

T1 = 110.0°C = 110.0 + 273.15 = 383.15 K T2 = -10.0°C = -10.0 + 273.15 = 263.15 K k1 = 4.4 * 10^5 k2 = 1.9 * 10^2 R = 8.314 J/(mol*K) (gas constant)

ln(k1 / k2) = Ea / R * (1/T2 - 1/T1)

ln(4.4 * 10^5 / 1.9 * 10^2) = Ea / 8.314 * (1/263.15 - 1/383.15)

Solving for Ea gives:

Ea = ln(4.4 * 10^5 / 1.9 * 10^2) * 8.314 / (1/263.15 - 1/383.15)

Calculate the above expression to get the activation energy Ea. Round your answer to 2 significant digits.