The following reaction is first order in N2O5: N2O5( g )NO3( g )+NO2( g ) The ra

Question

The following reaction is first order in N2O5:
N2O5(g)NO3(g)+NO2(g)
The rate constant for the reaction at a certain temperature is 0.053/s.

Part A:

Calculate the rate of the reaction when [N2O5]= 5.7×102 M .

Express your answer using two significant figures.

Part B:

What would the rate of the reaction be at the same concentration as in part a if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.)

Express your answer using two significant figures.

Part C:

Zero order?

Express your answer using two significant figures.

Explanation / Answer

The rate of the first order reaction is given by

Rate = K[N2O5], where K is the rate and [N2O5] represents the concentration of N2O5 at any time t

Part A

Rate = 0.053/s * 5.7 * 10^{-2} M = 3.021 * 10^{-3} Ms^{-1}

Two significant figures answer: 3.0 * 10^{-3} Ms^{-1}

Part B

If the reaction was a second order reaction, then the rate of reaction would be given as below

Rate = K[N2O5]^2 = 0.053 * 5.7 * 10^{-2} * 5.7 * 10^{-2} = 1.7297 * 10^{-4} Ms^{-1}

Two significant figures answer: 1.7 * 10^{-4} Ms^{-1}

Part C

If the reaction was a zero order reaction, then the rate of reaction would be given as below

Rate = K[N2O5]^0 = 0.053 * (0.057)^(0) = 0.053 Ms^{-1}

Two significant figures answer: 5.3 * 10^{-2} Ms^{-1}

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