Exercise 13.38 The following reaction is first order in Neos N20s (g) NO3 (g) NO

Question

Exercise 13.38 The following reaction is first order in Neos N20s (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 N20 5.6x10 2 M Express your answer using two significant figures. M/s Rate Submit My Answers Give Up 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 numenca value for the rate constant with the appropriate units Express your answer using two significant figures. M/s Rate Submit My Answers Give Up Part C Express your answer using two significant figures. M/s Rate Submit My Answers Give Up

Explanation / Answer

N2O5(g) ---> NO3(g) + NO2(g)

Part A The reactin is first order .hence

rate = K[N2O5]

     = 0.053*0.056 = 2.968*10^(-3) M/S

part B

if the reaction is 2nd order.hence

rate = K[N2O5]^2

     = 0.053*(0.056)^2 = 1.66*10^(-4) M/S

Part C
if the reaction is 2nd order.hence

rate = K[N2O5]^0

     = = 0.053*(0.056)^0 = 0.053 M/S

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