(A) Calculate the values of the rate constant k assuming that the reaction is fi
ID: 810200 • Letter: #
Question
(A)Calculate the values of the rate constant k assuming that the reaction is first order.
What is the value of k at 5 s?
What is the value of k at 10 s?
What is the value of k at 15 s?
What is the value of k at 25 s?
(B)Calculate the value of k assuming that the reaction is second order.
What is the value of k at 5 s?
What is the value of k at 10 s?
What is the value of k at 15 s?
What is the value of k at 25 s?
(C)Use your results from parts A and B above to decide what the order of the reaction is for your data. (Enter 1 or 2)
(D)What is the concentration of [A] at time t=69 s?
A reaction A right arrow B has the following time dependence for the concentration of [A] vs time. For t=(0 s, 5 s, 10 s, 15 s, 25 s) the concentration of [A]=(30.00 M, 12.45 M, 7.85 M, 5.74 M, 3.73 M). The initial concentration of [A] is the value at t=0 s. (A)Calculate the values of the rate constant k assuming that the reaction is first order. What is the value of k at 5 s? What is the value of k at 10 s? What is the value of k at 15 s? What is the value of k at 25 s? (B)Calculate the value of k assuming that the reaction is second order. What is the value of k at 5 s? What is the value of k at 10 s? What is the value of k at 15 s? What is the value of k at 25 s? (C)Use your results from parts A and B above to decide what the order of the reaction is for your data. (Enter 1 or 2) (D)What is the concentration of [A] at time t=69 s?Explanation / Answer
(A)
ln[A]=?kt+ln[A]o is the equation for first order kinetics.
k at 5s
ln[12.45] = -k(5) + ln[30.00]
k = 0.175 s^-1
k at 10s
ln(7.85) = -k(10) + ln(30.00)
k = 0.134 s^-1
k at 15s
ln(5.74) = -k(15) + ln(30.00)
k = 0.110 s^-1
k at 25s
ln(3.73) = -k(25) + ln(30.00)
k = 0.083 s^-1
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(B)
1/ [A]t = kt + 1/[A]o is the integral equation for second order reaction
k at 5s
1/12.45 = k(5) + 1/ 30.00
k = 9.40 x 10^-3 M/s
k at 10s
1/7.85 = k(10) + 1/ 30.00
k = 9.40 x 10^-3 M/s
k at 15s
1/5.74 = k(15) + 1/ 30.00
k = 9.40 x 10^-3 M/s
k at 25s
1/3.73 = k(25) + 1/ 30.00
k = 9.40 x 10^-3 M/s
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(C)
As, the k is constant at all times considering the results in part (B), the order of the reaction is SECOND ORDER.
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(D)
1/ [A]t = kt + 1/[A]o is the integral equation for second order reaction
1/[A]t = (9.40 x 10^-3)(69) + 1/[30.00]
[A]t = 1.47 M
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