Firstly we have to check whether the reaction is first order or not by using relation k1 = 1/t ln a/(a-x)
Calculated k1 is not constant in all cases.. Therefore this reaction will not be first order.
Determine the order of the reactant. aA bB Time [A] (s) 0 0.0100 4 0.0071 0.0055...
Determine the first half-life of the reaction. Determine the second and third half-lives. aA - bВ Time [A] (S) 0 0.0100 0.0071 8 0.0055 112 0.0045 16 0.0038
Determine the order of the reaction with respect to NOBr (g). Time (s) [NOBr] (M) ln [NOBr] 1 / [NOBr] (M-1) 0 0.01 -4.60 100.000 2 0.0071 -4.95 140.845 4 0.0055 -5.20 181.818 6 0.0045 -5.40 222.222 8 0.0038 -5.57 263.158 10 0.0033 -5.71 303.030
The concentration of reactant A (in M) in a reaction of A → products was monitored as a function of time. The experimental data were plotted in three graphs of [A] versus time, ln[A] versus time, and 1/[A] versus time as shown. Determine the reaction order. Reaction order graph Not enough information to determine the reaction order. Zero order First order Second order Not enough information to determine the reaction order. 0.8 0.6 0.4 0.2 3 -2 0 2 46...
Question 12 What is the concentration of reactant [A] at t = 15.00 s if A is 1st order, k = 0.428 s1 and the initial concentration of [A] = 8.30 M? Question 13. At what time (s) will [A] = 5.00 M if A is 2nd order, k = 0.428 M*s, and the initial concentration of [A] = 8.30 M? Question 14 Given the following rate law, find the half-life of the reactant o, if [0] = 0.322 M...
It takes 50.5 s for the concentration of reactant A in the second order reaction A ==> Products 0.84 mol L to half of it. to decrease from its initial value [A]o A) What is the rate constant of the reaction? B) What is the concentration of A after 32 s have passed? B) After what time will the concentration of A be [A]o 16?
18. From the reaction data below, determine whether the reaction is first-order or second-order. Time (S) Reactant (M) 6.67 1.59 0.74 0.39 0.16 25 a. First-order. b. Second-order. c. Zero-order. d. Cannot determine. 19. In the Question 18, what is the rate constant for the reaction? a. 0.12 b. 0.15 c. 0.24 d. 0.72 20. In the Question 18, what is the half-life for the reaction? a. 0.2 sec b. 0.6 sec c. 1.0 sec d. 1.3 sec
The half-life of a reaction, t1/2, is the time it takes for the reactant concentration [A] to decrease by half. For example, after one half-life the concentration falls from the initial concentration [A]0 to [A]0/2, after a second half-life to [A]0/4, after a third half-life to [A]0/8, and so on. on. For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t1/2=0.693k For a...
Use the following data to determine the order of reaction with respect to each reactant and the overall order: A + 5B + 6C + 3D + 3E Experiment [A] (M) [B] (M) [C] (M) -4 1 0.35 0.35 0.35 2 0.70 0.35 0.35 Initial Rate (M/s) 8.0 x 10 3.2 x 10-3 6.4 x 10-3 3.2 x 10-3 3 0.70 0.70 0.35 4 0.70 0.35 0.70 1) Order with respect to A = 2) Order with respect to B...
Velocity Vs. Time 10 8 6 Velocity , v, (m/s) 0 2 4 6 8 10 12 14 -4 -6 -8 Time, t, (s) a) Determine the average velocity of the object between 4.0 and 8.0 s. Over what time interval(s), if any, is the object decelerating (slowing down)? b) At what time(s), if any, does the object remain at rest?
4. Determine the standard cell potential for each of the electrochemical cells. 2Ag(s) + Pb2+(aa) 2" (ac) + 2(s) a. 2Ag1+(aa) + Pb(s) 2(g) (ac) 2+ (ag)