Q2/ A) The following reaction was monitored as a function of time: A → B+CA plot of In[A] versus time yields a straight line with slope=- 0.0045 s1) What is the value of the rate constant, k, for this reaction at this temperature?2) What is the half life?3) If the initial concentration of A is 0.250 mol.L' what is the concentration of A after 225 s?B)4A2+4B2 +8ABAH= 73 kJExplain the effect of the following on the reaction equilibirum:(1) Removed [A] (2) IT (3) ↑ PC) For a system in which the following reaction occurs: CH4 + H20 CO + 3H2Assume there are present initially 3 mole CH, 1 mol H20, 2mol CO and 4 mol H2.Determine expreession for the mol fraction yi as afunction of (H20 and H2)?

Answered: Image /qna-images/answer/ea8e213f-bf94-427e-85dd-3ab06640721c.jpg

Q2/ A The following reaction was monitored as a function of time: A+ B+C A plot of In[A] versus time yields a straight line with slope=-0.0045 s 1) What is the value of the rate constant, k, for this reaction at this temperature? 2) What is the half life? 3) If the initial concentration of A is 0.250 mol.L' what is the concentration of A after 225 s?

Q2/ A The following reaction was monitored as a function of time: A+ B+C A plot of In[A] versus time yields a straight line with slope=-0.0045 s 1) What is the value of the rate constant, k, for this reaction at this temperature? 2) What is the half life? 3) If the initial concentration of A is 0.250 mol.L' what is the concentration of A after 225 s?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

7. Given the following reaction graph for reactant SO₂Cl2. -2.3 a. What is the reaction order for SO₂Cl2 on the graph? b. What is the initial concentration of SO₂Cl2 in the reaction shown? () [ c. Calculate the rate constant, k, for the reaction. e. Calculate the half-life of the reaction. -2.4 -2.5- -2.6 -2.7 -2.8 -2.9 -3 -3.1 -3.2- 0 1.0 x 104 d. Solve for the amount of SO₂Cl2 that is present after 5.0 x 104 seconds. 2.0 x 10² time (s) f. How long would it take for only 20% of the original amount of SO₂Cl2 to remain? 3.0 x 104 4.0 x 104
(c) A reaction between substances R and S was second order with respect to R and second order with respect to S. S-or x 8.1 0.3 At a given temperature, the initial rate of reaction was 1.20 x 10-3 mol dm-3 s-1 when the initial concentration of R was 1.00 x 10-2 mol dm-3 and the initial concentration of S was 2.45 x 10-2 mol dm-3 acom ton Scor 0.8 Calculate a value for the rate constant, k, for the reaction at this temperature. Give the units for k rose ni to nollbeen to stist leitini ert worla of SeldsT otalama) (B) S eldsT amb tom \\ els fallinl Ot *8.1 Inomheqx3
A reaction is second order with respect to reactant "A" and has a rate constant of 2.97 x 10-2 M-1s-1. If the initial concentration of A is 0.100 M, what will the concentration drop to after 30.0 minutes? 6.06 x 10E(-25) M 9.18 x 10E(-2) M 1.58 x 10E(-2) M 1.01 x 10E(-26) M
2HIg) --> H2g) +l2ls) The above reaction is zero order with respect to HI. The rate constant was found to be 1.2 X 10-4 mol/L.s. If the intial concentration of HI was 0.250 mol/L. Cal culate the comcentration of HI at 13.6 minutes after the start of the reaction (You answer should be to 2 d.p. eg., 0.45 Answer:
Calculate the instantaneous rate of the reaction (M/s), A + B ->C , where the rate constant is 5.64 x 102 M-1s-1? A has 0.054M concentration and the concentration of B is 0.043 M and the reaction is in second order relative to A and zero order relative to B. Balance the reaction as followsT TeO32- + N2O4 + H2O -> Te + NO3- + H+
Ch. 14, 54. A reaction indicated by the chemical equation below 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 0.055 M-¹ s-¹. a) Determine the rate constant for this reaction (assume the temperature does not change). b) Write the rate law equation for the reaction. c) What is the half-life of the reaction if the initial concentration of AB is 0.550 M? d) If the initial concentration of AB is 0.250 M, what are the molar concentrations of A and B after 75 s?
what is the answer?
b Calculate the rate of the reaction when N2O5] is 1.0 M. Rate = M/s %3D
which one is correct?
For a reaction with the following rate expression: rate = k[A], a plot of which of the following is a straight line? a) [A] versus time d) [A] versus 1/time b) ln[A] versus time e) ln[A] versus 1/time c) 1/[A] versus time
None
* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit