NEED HELP FAST!!!!

Question

The reaction 

C4H8(g)⟶2C2H4(g)

has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, 𝑘, is 6.1×10−8 s−1. 

What is the value of the rate constant at 790.0 K?

Answer 1

Instead of using A (frequency factor), you can use a variation of the Arrhenius equation.

Variation of the Arrhenius Equation is used to find the value of k at a different temperature:

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

k2 = ?

k1 = 1.6x10-8

Ea = 262 kJ/mol

R = 8,314 J/mol-K = 0.008314 kJ/mol-K (use this value)

T1 = 600 K

T2 = 790 K

Solve for k2