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Question: The following is the overall reaction for a multi-step process:

2 N₂O₅ (g) --> 4 NO₂ (g) + O₂ (g)

If the variation in N₂O₅ concentration over time for the overall reaction is shown below, what is the rate law for the reaction?

80 70 60 50 (w) (ON 40 Z 30 20 10 0 0 50 200 250 100 150 Time (hours) Items Conjunctions Required Conclusion Reasoning Space to Build Argument The first half-life of this reaction is approximately 53 hours 1 because 1 Rate = k[N205] The plot provides the rate of the reaction 2 Rate = k[N20512 2 because 3 because N2O5 has a coefficient of two in the reaction Rate = k[NO_110,1 SO 4 Rate = k[N OINO2102] The half-life is the length of time it takes for the initial concentration to decrease by half 5 SO 5 Rate = k[N2012/NO, 1102] In this reaction, N, O, is a gas 6 so The first and second half-lives are equal in length 7 therefore The balanced overall reaction is not relevant for determining the rate law 8 therefore 9 and For an elementary step, the reaction order matches the reactant coefficients 10 and The reactant concentration does not decrease linearly 11 and 12 but A rate law includes the concentration of each reactant raised to its reaction order 13 but The half-life for a first order reaction is constant over time 14 but 15 but In this reaction, a single reactant decomposes to give two different products Custom: Custom