concentrationof A is the value at t = 0s. (-1A)Calculate the values of the rate constantk assuming that the reaction is first order.What is the value of k at 5 s? s¯¹ What isthe value of k at 10s ? 00.080 S What isthe value of k at 15s ? s What is the-1value of k at 25s ? s¹ (B)Calculate the-1-1value of k assuming that the reaction issecond order. What is the value of k at5s ? M¹¹ What is the value of k at-110s ? M¹¹ What is the value of k atS15s M¹¹ What is the value of k atS-125s ? M¹s1¹ (C) Use your results fromparts A and B above to decide what theorder of the reaction is for your data. (Enter 1 or 2) (D) What is the concentrationof A at time t = 61s ? A reaction AB has the following time dependence for the concentration of [A] vs time. For t=(0 s, 5 s, 10 s, 15 s, 25 s) the concentration of [A] =(30.00 M, 20.01 M, 13.35 M, 8.90 M, 3.96 M). The initialconcentration of [A] is the value at t=0 s.(A)Calculate the values of the rate constant k assuming that the reaction is first order.What is the value of k at 5 s? 0.080What is the value of k at 10 s? 0.080What is the value of k at 15 s? 0.081What is the value of k at 25 s? 0.081(B)Calculate the value of k assuming that the reaction is second order.What is the value of k at 5 s? 0.0032M¹s1M¹5 1What is the value of k at 10 s? 0.0042What is the value of k at 15 s? 0.0058M¹51What is the value of k at 25 s? 0.0088M-¹51s1$1s1$1MY NOTES(C)Use your results from parts A and B above to decide what the order of the reaction is for your data. (Enter 1 or 2) 1(D)What is the concentration of [A] at time t=61 s?M

The objective of the question is toa) Calculate the values of the rate constant assuming the…

concentration of A is the value at t = 0s. ( A)Calculate the values of the rate constant k assuming that the reaction is first order. What is the value of k at 5 s? s What is -1 -1 the value of k at 10s ? 00.080 s¹ What is S -1 -1 the value of k at 15s ? s What is the value of k at 25s ? s¯¹ (B)Calculate the value of k assuming that the reaction is second order. What is the value of k at 5s ? M¹¹ What is the value of k at -1 S -1 10s ? M¹¹ What is the value of k at S 15s M¹¹ What is the value of k at -1 .-1 25s ? M¹s¹ (C) Use your results from parts A and B above to decide what the order of the reaction is for your data. ( Enter 1 or 2) (D) What is the concentration of A at time t = 61s ?

concentration of A is the value at t = 0s. ( A)Calculate the values of the rate constant k assuming that the reaction is first order. What is the value of k at 5 s? s What is -1 -1 the value of k at 10s ? 00.080 s¹ What is S -1 -1 the value of k at 15s ? s What is the value of k at 25s ? s¯¹ (B)Calculate the value of k assuming that the reaction is second order. What is the value of k at 5s ? M¹¹ What is the value of k at -1 S -1 10s ? M¹¹ What is the value of k at S 15s M¹¹ What is the value of k at -1 .-1 25s ? M¹s¹ (C) Use your results from parts A and B above to decide what the order of the reaction is for your data. ( Enter 1 or 2) (D) What is the concentration of A at time t = 61s ?

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 14Q: Each of the statements given below is false. Explain why. a. The activation energy of a reaction...

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Similar questions

Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.
The activation energy for the decomposition of cyclobutane (C4H8) to ethylene (C2H4) is 261 kJ/mol. If the system produces ethylene at the rate of 0.043 g/s at 500C, what is the rate if the temperature increases to 600C?
Each of the statements given below is false. Explain why. a. The activation energy of a reaction depends on the overall energy change (E) for the reaction. b. The rate law for a reaction can be deduced from examination of the overall balanced equation for the reaction. c. Most reactions occur by one-step mechanisms.
11.34 Rate data were obtained at 25°C for the following reaction. What is the rate law expression for this reaction? A + 2B — C + 2D Expt Initial [A] (mol L-’) Initial [B] (mol L_1) Initial Rate ofFormation of C (mol L-1 min-1) 1 0.10 0.10 3.0 X 10~4 2 0.30 0.30 9.0 X 10"4 3 0.10 0.30 3.0 X 10~4 4 0.20 0.40 6.0 X 10"4
Consider a 5.000 M solution of the hypothetical com- pound R. Its decomposition is a second-order reaction and its activation energy is 57.6 kJ/mol. At 759C, the half-life of the 5.000 M solution is 8.49 h. What is the half-life of the same solution at 700C (3 significant figures)?
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?