For the reaction:
2n2o5(g) → 4no2(g) + o2(g) the rate law is: (δ[o2]/δt) = k[n2o5] at 300 k, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kj/mol. what is the half-life at 310 k? (hint: use rate law expression to determine the reaction order → solve for k1 at 300 k using the corresponding half-life expression → use two-point arrhenius equation to solve for k2 at 310 k → use the half-life expression again to solve for half-life at 310 k)