The problem gave us the values for activation energy, 2 temperatures, and 1 rate constant k. Now it asks us another k value at a certain temperature. Based on these, we can say that we would need to use the 2 point form of the Arrhenius equation.
The following reaction has an activation energy of 262 kJ/mol.
C4H8(g) → 2C2H4(g)
At 600.0 K the rate constant is 6.1 x 10-8 s-1. What is the value of the rate constant at 725.0 K?
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