Reaction Kinetics 1) Write a basic form of the rate law for the following reacti

Question

Reaction Kinetics

1) Write a basic form of the rate law for the following reaction.

ClO4^- + 8Br^- + 8H^+ = Cl^- + 4Br2 + 4H2O

2) If doubling the concentration of perchlorate ion in the reaction above causes the rate of reaction to quadruple, what is the order of reaction with respect to perchlorate ion?

3) A plot of In(Rate) vs. 1/T for the above reaction gave a straight line with a slope of -4545. What is the activation energy for this reaction?

4) By what factor would the rate of reaction increase if you doubled [I^-1] and increased the temperature of he reaction by 10 degrees C at the same time? Explain your answer

5) Use the following data to determine the rate law and rate constant for the reaction:

NH4^+ + NO2^-1 = N2 + 2H2O.

Explanation / Answer

1) rate law = k [ClO4-]x [Br-]y [H+]z

2) order with respect to perchlorate ion = 2

rate = k [ClO4-]x

4      = k (2)x

22 = k (2)x

x =2

3) slope = -Ea / R = -4545

Ea = 4545 R

Ea = 4545 x 8.314 x 10^-3 kJ

Ea = 37.78 kJ

activation energy = Ea = 37.78 kJ

4) rate becomes 2 times.

for every raise in 100C temperature rate will increase 2 times

5) rate law = k [NH4+] [NO2-]

    by solving data 1 , 2 we get order with respect to NO2- =1

by solving data 3,4 we get order with respect to NH4+ =1

6.98 x 10^-7 = k (0.0184)(0.098)

k = 3.87 x 10^-4

rate constant = 3.87 x 10^-4 M-1s-1

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