A. The reactant concentration in a zero-order reaction was 5.00×10 ?2 M after 18

Question

A. The reactant concentration in a zero-order reaction was 5.00×10?2M after 180 s and 3.50×10?2Mafter 310 s . What is the rate constant for this reaction?

B. What was the initial reactant concentration for the reaction described in Part A?

C. The reactant concentration in a first-order reaction was 6.10×10?2M after 30.0 s and 7.20×10?3Mafter 85.0 s . What is the rate constant for this reaction?

D. The reactant concentration in a second-order reaction was 0.320 M after 240 s and 6.40×10?2Mafter 700 s . What is the rate constant for this reaction?

Please show the work and the correct untis for each! thank you!

Explanation / Answer

A) In zero order reaction

rate of the reaction = k [reactant]^0

rate of the reaction = K

(CHANGE IN CONCENTRATION)/(CHANGE IN TIME) = K

(5..0*10^-2 - 3.50*10^-2)/(310-180) = K

K= 1.15*10^-4 M S^-1

B) K = [a]-[a-x]/t

1.15*10^-4 = [a]-[5.00*10^-2]/180

    [a] = 7.07*10^-2 M

WHERE a = initial concentration of the reactant

c) K1 = (2.303/t2-t1) log(c1/c2)

        = (2.303/(85-30)) log(0.0610/0.00720)

        = 4.330*10^-2 s^-1

d)

for second order reaction

rate of the reaction = k [reactant]^2

rate of the reaction = K[reactant]^2

(0.320-0.0640)/(700-240) = K[0.320]^2

k= 5.43*10^-3 mole^-1. lit .s^-1

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