The Kinetics for the reaction 2 A + 3 B rightarow C + 2 D were studied at 20 deg

Question

The Kinetics for the reaction 2 A + 3 B rightarow C + 2 D were studied at 20 degree C, and the following data were obtained by monitoring the rate of consumption of A. If it takes t seconds for A to be consumed, the initial rate for the consumption of A is equal to the initial concentration of A divided by the product of the time required for A to be consumed and the stoichiometric coefficient of A. rate = -1/a (Delta [A]/Delta t) = 1/2 ([A]_initial/t_consumption of A) Calculate the initial concentrations of A and B, and the initial rate for each Experiment. Enter the results in the table below. Show all calculations.

Explanation / Answer

Total volume of the reaction = volume of A + volume of B + volume of water added

for all three experiments total volume = 50.0 mL

Initial conc. for A in exp. 1 = 0.0080 x 10.0 / 50 = 0.0016 M

Initial conc. for A in exp. 2 = 0.0080 x 20.0 / 50 = 0.0032 M

Initial conc. for A in exp. 3 = 0.0080 x 10.0 / 50 = 0.0016 M

Initial conc. for B in exp. 1 = 0.2 x 10.0 / 50 = 0.04 M

Initial conc. for B in exp. 2 = 0.2 x 10.0 / 50 = 0.04 M

Initial conc. for B in exp. 3 = 0.2 x 30.0 / 50 = 0.12 M

Therefore

initial rate in experiment 1 = 0.0016 M/ 2 x 82 s = 9.76 x 10-6 M/s

initial rate in experiment 2 = 0.0032 M/ 2 x 41 s = 3.90 x 10-5 M/s

initial rate in experiment 3 = 0.0016 M/ 2 x 82 s = 9.76 x 10-6 M/s

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