Chemistry Kinetics Help

Question

The reaction 

has an activation energy of  At  the rate constant,  is  What is the value of the rate constant at 

Answer 1

Arrhenius equation:

ln k₂/ln k₁ = Ea/R(1/T₁ - 1/T₂)

k₁ = 6.1x10^-8 s^-1

T₁ = 600 K

k₂ = ?

T₂ = 800K

Ea = 262 kJ/mol = 262000 J/mol

R = 8.314 J/mol-K

ln k₂/ln 6.1x10^-8 = 262000/8.314 (1/600 - 1/800)

I'll leave the math to you to solve for k₂