For the reaction: 2N2O5(g) ? 4NO2(g) + O2(g) the rate law is:(?[O2]/?t) = k[N2O5] At 300 K, the half-life is 2.50 × 104 secondsand the activation energy is 103.3 kJ/mol. What is the half-life at310 K? (Hint: Use rate law expression to determine the reactionorder ? solve for k1 at 300 K using the corresponding half-lifeexpression ? use two-point Arrhenius equation to solve for k2 at310 K ? use the half-life expression again to solve for half-lifeat 310 K)

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For the reaction 2NO5g 4NOg Og the rate of form... View the full answer