The decomposition of hydrogen iodide gas to hydrogen gas and iodine gas occurs a

Question

The decomposition of hydrogen iodide gas to hydrogen gas and iodine gas occurs at a rate of 1.16x10^-3 at 427 degrees Celsius, and at a rate of 3.52x10^-7 at 283 degrees Celsius.
(a) Calculate the activation energy of this reaction, in kJ/mole. (b) what is the temperature in Celsius of a reaction that has a rate constant of 2.19x10^-4 m^-1s^-1 (c) What is the rate constant if the temperature is 537K? The decomposition of hydrogen iodide gas to hydrogen gas and iodine gas occurs at a rate of 1.16x10^-3 at 427 degrees Celsius, and at a rate of 3.52x10^-7 at 283 degrees Celsius.
(a) Calculate the activation energy of this reaction, in kJ/mole. (b) what is the temperature in Celsius of a reaction that has a rate constant of 2.19x10^-4 m^-1s^-1 (c) What is the rate constant if the temperature is 537K?
(a) Calculate the activation energy of this reaction, in kJ/mole. (b) what is the temperature in Celsius of a reaction that has a rate constant of 2.19x10^-4 m^-1s^-1 (c) What is the rate constant if the temperature is 537K?

Explanation / Answer

ln 3.52 ×107 / 1.16x10^-3 = Ea / 8.314 ( 1/700 -1/556)

-8.1 x 8.314 / -3.69988 x 10-4 = Ea

Ea = 18.2 x 104 Joules

Then in the same we apply for another temerature for c

ln k1 / 1.16x10^-3 = 18.2 x 104 / 8.314 ( 1/700 -1/537)

ln k1 / 1.16x10^-3 = -9.49028

Log k1 = - 7.055

rate constant k = 8.7933 x 10-8 Sec -1 at 537 K

Calculation b

ln 2.19x10^-4 / 1.16x10^-3 = 18.2 x 104 / 8.314 ( 1/700 -1/T1)

to solve aboce equation will get T1

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