Help, how do you solve this?

Activation energy: Eₐ = 65.25 kJ/mol = 65250 J/mol
Gas constant, R = 8.314 J/(mol K)
At T₁ = 303 K, k₁ = kₒ
At T₂ = ?, k₂ = 7kₒ

Arrhenius equation: ln(k₁/k₂) = (Eₐ/R) × [(1/T₂) - (1/T₁)]
ln[kₒ/(7kₒ )] = (65250/8.314) × [(1/T₂) - (1/303)]
(1/T₂) - (1/303) = (8.314/65250) ln(1/7)
(1/T₂) = (1/303) + (8.314/65250) ln(1/7)
The required temperature, T₂ = 1 / [(1/303) + (8.314/65250) ln(1/7)] = 328 K (to 3 sig. fig.)