If the activation energy for a given compound is found to be 42.0 kj/mol, with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 k? a) 2.9 × 10-4 s-1. b) 7.4 × 10-4 s-1. c) 1.4 × 109 s-1. d) 4.6 × 10 5 s-1. e) 3.5 × 103 s-1.

The problem is related to Arrhenius' equation that correlates rate constant and temperature using activation energy  and frequency factor as constants. 
k = ko e ^ -E/RT where E is the activation energy and ko as frequency factor. substituting, 
k = 8.10x10^10 e ^ -42.0 x 10^3 J/mol-/8.314 *298 K
k = 3474.52 s-1