The integrated rate laws for zero, first-, and second-order reaction may be arra

Question

The integrated rate laws for zero, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mx + b. The reactant concentration in a zero-order reaction was 0.100 M after 170 s and 4.00 times 10^-2 M after 340 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. What was the initial reactant concentration for the reaction described in Part A? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. [A]_0 =

Explanation / Answer

PartA

Let us assume initial concentration is 0.1M which is [A]0

Reaction time is t =170s

Concentration after 170s = 4×10^-2M

applying these values in integrated rate law of zero order we can get k

[A] = -kt + [A]0

4×10^-2 M =- k × 170 s + 0.1 M

-k = (4× 10^-2M - 0.1 M)/170s

k =3.53 × 10^-4M/s

Part B

k = 3.53 × 10^-4M/s

[A]0 = ?

[ A] = 0.1 M

t = 170s

Applying these values in above equation

[ A ] = - k t + [ A]0

0.1M = - ( 3.53 × 10^-4 M/s × 170s ) + [A]0

[A]0 = 0.1 M + 0.0600M

= 0.1600M

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