In an experiment to determine the rate law, the rate of the reaction was determi

Question

In an experiment to determine the rate law, the rate of the reaction was determined to be 88.7 Ms-1 when [C5H10] = 0.100 M and [O3] = 7.65E-3 M. From this experiment, the rate constant is _______________M-1s-1.

Rate = ___________________ A) The reaction of UO2^+ with hydrogen ion in aqueous solution 2 UO2^+ + 4 H^+ Arrow U^4+ + UO2^2+ + 2 H2O is second order in UO2^+ and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =_______________ B) The ozonization of pentene in carbon tetrachloride solution at 25 degree C C5H10 + O3 Arrow C5H10O3 is first order in C5H10 and first order in O3. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = ___________________ In an experiment to determine the rate law, the rate of the reaction was determined to be 88.7 Ms^-1 when [C5H10] = 0.100 M and [O3] = 7.65E-3 M. From this experiment, the rate constant is _______________M^-1s^-1.

Explanation / Answer

A)

Rate = k [UO2+]^2 [H+]

B)

Rate = k [C5H10] [O3]

C)

Rate = 88.7 M/s

Rate law is, Rate = k[C5H10][O3]

88.7 = k (0.100) ( 7.65 x 10^-3)

k = 115947.71

k = 1.16 x 10^5 M^-1 s^-1

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