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For the decomposition of hydrogen iodide, 2HI â H₂ + I₂, the rate constant is 9.51Ã10^-9 M^-1s^-1 at 500 K and 1.10Ã10^-5M^-1s^-1 at 600 K. What is the value of the activation energy, E_a, in kJ/mol?

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Related questions

The HI decomposition reaction

2HI âãH2 + I2

Ea = 182kj/mole

And at 700 degree c , the rate constant is 1.57x 10-3 M-1S-1

What is the rate constant at the 600 degree c?

I use log k2/k1 = -Ea/Rx2.303 (1/T2 - 1/T1)

But the answer is wrong

Answer is 1.19x10-3 M-1S-1

The rate constant for the formation of hydrogen iodide from the elements

H₂(g) + I₂(g) ---> 2HI(g)

is 2.7 x 10^-4 L/(mol-sec) at 600 K and 3.5 x 10^-3 L/(mol-sec) at 650 K.

1. Find the activation energy

2. Calculate the rate constant at 700K.

The activation energy for the decomposition of HI(g) to H₂(g) and I₂(g) is 200 kJ/mol. The rate constant at 600 K is 6.82 x 10^-7L/mol·s. What is the rate constant at 820 K?

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