This is a second order reaction having equation : 1 / [AB]=1 / [AB] 0 +kt Slope

Question

This is a second order reaction having equation :
1 / [AB]=1 / [AB]0+kt

Slope = rate constant = 5.2 * 10^(-2) (Ms)^(-1)

Half life time is the time it takes for reactant to decay to half of its original value;

Putting AB= AB0/2

We get :

t1/2=1/ (k *[AB0]

= 1 / (5.2 * 10^(-2) * 0.59 )

=32.59 seconds

PARTC : Half life = 33 seconds

PART D :
1 / [AB]=1 / [AB]0+kt

After 80s :

1 / [AB]=1 / 0.23 +5.2 * 10^(-2) * 80

=4.347 + 4.16 = 8.507

[AB] = 0.1175 M
Since , ABA+B stotiometric coeffeicients are 1 only

[AB] lost = 0.23 - 0.1175 = .1125 M is [A] and [B] inccreased
PART D : [A] = [B] = 0.11 M

Explanation / Answer

The following reaction was monitored as a function of time:
ABA+B
A plot of 1/[AB] versus time yields a straight line with slope 5.2×102 (Ms)1 .

You may want to reference (Pages 568 - 575) section 15.5 while completing this problem.

iPad 5:05 AM * 35% a session.masteringchemistry.com + D Now | UMass L..Learning Mana. Significant Figu. Chegg Study Assignments MasteringCh... Write the rate law for the reaction. O Rate= k Rate = k [AB) Rate = k AB12 O Rate = k [AB13 Previous Correct Second order reactions produce a straight line when 1/[AB is plotted as a function of time. Second order reactions are described by the equation Rate-k [Reactant Part C What is the half-life when the initial concentration is 0.59 M? Express your answer using two significant figures. SubmitP Previous Answers Request Answer Incorrect; Try Again; 5 attempts remaining Part D If the initial concentration of AB is 0.230 M.and the reaction mixture initially contains no products, what are the concentrations of A and B after 80 s? Express your answers numerically using two significant figures, separated by a comma. Aj, [B] Submit Provide Feedback Next >

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