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

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

ln(k2/k1) = -262/0.008314 (1/790 - 1/600)

ln(k2/k1) = 12.6

k2/k1 = 296,559

k2/1.6x10^-8 = 2.97x10⁵

k2 = 4.75x10^-3 s^-1