Question

54. This reaction was monitored as a function of time: AB —— A + B A plot of 1/[AB] versus time yields a straight line with a slope of +0.55/M.s. a. What is the value of the rate constant (k) for this reaction at this temperature? b. Write the rate law for the reaction. c. What is the half-life when the initial concentration is 0.55 M? d. If the initial concentration of AB is 0.250 M, and the reaction mixture initially contains no products, what are the concert trations of A and B after 75 s?

I need help with a. b. c. and d. please. thank you

Answer 1

Given reaction AB - A+B slope = +0.55 Mist is a) We know that for and order reaction, integrated rate law [A] cade+ kt when we compare this equation with straight line equation y = mx + c we get slope = k . so rate constant = 0.55 Mist b) as the given reaction is and order reaction so rate law is rate = K[AB]? ) for and order reaction t1/2 = K[ALO - Oss Madset x 0.55m - 0.3015 s t2 = 3.3058 sec. CSScanned with CamScanner

d) [AB] = 0.25m ; t = 75 sec. - +0.55m-s x 75 ser. 0.25 - TAB 410-1 & 41.25 M1 0.0221 M . [AB] = 45.25M-1 - now . initial change final AB 0.25 0.0221 = 0.25M-X = 0.0221 M i x = 0.25M-0.0221M = 0.2279 30, concentration of A and B af t=75 sec is 0.2279 M Scanned with CamScanner