Determine the rate law and the value of k for the following reaction using the d

Question

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5 (g) = 4 NO2 (g) + O2 (g) [N2O5]i (M), Initial Rate (M^-1 s^-1) 0.093, 4.84 x 10^-4 0.186, 9.67 x 10^-4 0.279, 1.45 x 10^-3 Answer Choices: A) Rate = 5.6 x 10^-2 M^-1 s^-1 [N2O5]^2 B) Rate = 6.0 x 10^-1 M^-2 s^-1 [N2O5]^3 C) Rate = 1.6 x 10^-3 M^1/2 s^-1 [N2O5]^1/2 D) Rate = 1.7 x 10^-2 M^-1/2 s^-1 [N2O5]^3/2 E) Rate = 5.2 x 10^-3 s^-1 [N2O5] Please help me. I'm so lost and have no idea how to solve this problem. Please show work and explanations. Thank you.

Explanation / Answer

C) Rate = 1.6 x 10^-3 M^1/2 s^-1 [N2O5]^1/2

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