The reactant concentration in a zero-order reaction was 6.00×10 2 M after 200 s

Question

The reactant concentration in a zero-order reaction was 6.00×102M after 200 s and 4.00×102Mafter 365 s . What is the rate constant for this reaction?

Express your answer with the appropriate units.

Part B

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

part c The reactant concentration in a first-order reaction was 9.90×102M after 30.0 s and 1.00×102Mafter 65.0 s . What is the rate constant for this reaction?

Part D

The reactant concentration in a second-order reaction was 0.640 M after 100 s and 6.30×102M after 880 s . What is the rate constant for this reaction?

Express your answer with the appropriate units. Include an asterisk to indicate a compound unit with mulitplication, for example write a Newton-meter as N*m.

Order Integrated Rate Law Graph Slope 0 [A]=kt+[A]0 [A] vs. t k 1 ln[A]=kt+ln[A]0 ln[A] vs. t k 2 1[A]= kt+1[A]0 1[A] vs. t k

Explanation / Answer

K = a-(a-x)/(t2-t1)
a = 6.00*10^-2
(a-x) = 4.00*10^-2
t1 = 200s , t2 = 365s
K = [(6-4)*10^-2] / (365 - 200)

K = 2*10^-2 / 165
K   = 0.012*10^-2 m/sec.
................................................

PartB
0.012*10^-2 = [a - (6*10^-2)] / 200
[a] = 8.42*10^-2M

..................................................

PartC
K = 2.303/(t2-t1) log[(a-x1)/(a-x2)]

K = 2.303/(65-30) log[9.9*10^-2/1*10^-2]

K = 6.55*10^-2 sec^-1
........................................................
PartD

K = 1/(t2-t1)[1/(A-x2) - 1/(A-X1)]

K = 1/(880-100) [1/6.3*10^-2 - 1/0.64]

K = 1.835*10^-2 M^-1 * sec^-1

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