Using Integrated Rate Laws | Integrated rate equation [A]--kt + [Alo | Linear |

Question

Using Integrated Rate Laws | Integrated rate equation [A]--kt + [Alo | Linear | k = graph Aslope Ms[Al,/2k | Units | Half- of k life Order Rate Law 0 Rate-k In2 /k Given the following graphical analysis answer the following questions for the reaction C4H8 2C2H4. 1. 0.000 20 40 60 80 100 120 0.200 -0.400 c. What is the concentration of C4Hs InICHal, M 0600 0.800 [ slope=-6.64E-3 | a. b. What is the rate law? What is rate constant with units? after 45 sec, if the initial concentration is 0.525 M? What is the half-life for the reaction, if the initial concentration is 0.525 M? d. 1.000 1.200 Time,s 2. The rearrangement reaction CH3NEC CHC N is first order with a rate constant of 5.11E-5 s. The initial concentration of CH3NEC is 0.0340 M. What is the concentration after 2.00 hours? Determine the time in minutes that must elapse to reach a CH3NEC concentration of 0.0300 M. a. b. The simple decomposition reaction, AB(g) A(g) + B(g), is a second order reaction with a rate constant of 0.20 Ms at 25 °C. 3. How long will it take for the concentration of AB to reach 1/3 of the initial concentration of 1.50 M? What the half-life for this reaction the initial concentration of 1.50 M? What is the half-life once the concentration reactions 0.50 M AB? What do you notice about the answers to b and c? a. b. c. d. 4. The first-order rate constant at 20 °C for the decomposition of a certain antibiotic in water is 1.65 yr a. What is the concentration of a solution initially at 6.0E-3 M after 3 months? b. After I year? c. How long will it take for the concentration to drop to 1.0E-3 M?

Explanation / Answer

1)

a)

Rate=k[A]

b)

Rate constant: It is a coefficient of proportionality relating the rate of a chemical reaction at a given temperature to the concentration of reactant (in a unimolecular reaction) or to the product of the concentrations of reactants.

k=6.64*10^-3 s^-1

c.)

ln A = ln Ao - Kt

ln A = ln 0.525 - (6.64 x 10-3) x 45

ln A = -0.9432

[A]= 0.3894 M

d.)

half life reaction = 0.693/K ( reaction is of first order)

= 0.693/6.64 x 10-3

= 104.37 s

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