1. Given the following data, determine the orders (m and n) with respect to the concentrationsof A and B in the reactionOrders:[A]0.020 M0.020 M0.010 M0.010 Mm=A+BproductsRate = k[A][B]"[B]0.020 M0.010 M0.020 M0.010 Mn =Time for reaction19 sec19 sec76 sec76 secWhat time would you predict if both concentrations of A and B were made to be 0.040 M?

The objective of the question is to determine the order of the reaction and predict at what time the…

1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction [A] 0.020 M 0.020 M 0.010 M 0.010 M A+B products Rate = k[A][B]" [B] 0.020 M m= 0.010 M 0.020 M 0.010 M Time for reaction 19 sec 19 sec n = 76 sec Orders: What time would you predict if both concentrations of A and B were made to be 0.040 M? 76 sec

1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction [A] 0.020 M 0.020 M 0.010 M 0.010 M A+B products Rate = k[A][B]" [B] 0.020 M m= 0.010 M 0.020 M 0.010 M Time for reaction 19 sec 19 sec n = 76 sec Orders: What time would you predict if both concentrations of A and B were made to be 0.040 M? 76 sec

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

kinetic data for the following reaction was determined experimentally; 2NO(g) + Chlg) - 2NOCI(g) Experiment number [Ch). M 0.20 [NO). Initial rate of reaction M 0.10 0.30 M/s 0.63 5.70 0.20 0.80 2 0.10 2.58 The orders of the reaction with respect to NO and Cly are respectively. and O two and one, respectively. O one and two, respectively. O three and one respectively. O one and three, respectively,
Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137
7. A student is studying the reaction A + B→ C and measures the following kinetic data. [A] (M) [B] (M) Rate (M/s) Experiment 1 0.025 M 0.033 M 0.100 M/s 0.025 M 0.050 M 0.229 M/s 3 0.040 M 0.050M 0.366 M/s From this data determine the rate law for the reaction and find the value of the rate constant. Make sure you have the correct units on the rate constant.
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
Consider the following balanced chemical equation: H₂O2 (aq) + 31 (aq) + 2 H* (aq) → 13¯ (aq) + 2 H₂O (1) In the first 49.9 seconds of the reaction, the concentration of 13 increased from 0.692 M to 0.93 M. What is the average reaction rate over this time interval (in mol L-¹ s-¹)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
X2 + Y₂ → 2Z R = k[Y₂] Trial [X₂]. (M) [Y₂], (M) Initial Rate (M/hr) 1 0.100 0.100 2.15 x 10-3 2 0.100 0.300 6.45 x 10-3 3 0.300 0.200 4.30 x 10-³ What is the rate constant for the reaction given the rate law and data? k = [?] Enter the answer choice number. Rate Law Expression Enter
Do not give handwriting solution.
The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1
Consider the following chemical reaction A - B+ C A plot of 1/A vs. time (in seconds) is a straight line with a slope of 0.0040 Ms1 (OR per molar per second). Calculate the time required, in seconds, for the concentration of A to decrease to 1.03 M when the initial concentration of A is 2.87 M
Consider the reaction: A - → 2C The concentration of reactant A and product B were monitored at the same time interval. Time t, Minutes Molar Concentration A, [A] Molar Concentration C, [C] 0 2.40 0.00 2.00 2.20 0.40 4.00 2.00 0.80 1. Calculate the change in the concentration of A per unit time (M/min) from time (t=0 min) to time (t=2.00 min). Mark the box with an X to identify your choice of the correct answer. (5 pts) + 0.20 M/min + 0.10 M/min - 0.20 M/min - 0.10 M/min
What is the rate of the reaction when A=0.43M and B=0.31M?
[item#2a] *refer to the photo below*