6. Consider the following chemical reaction:2 NO + 2 H2 → N2 + 2 H20The following data was collected over three experiments:Experiment[NO] (M)[H2] (M)Initial Rate (mol L1 s1)110.0 x 1032.0 x 10-35.0 x 10-5210.0 x 1034.0 x 10-310.0 x 10514.0 x 1032.0 x 10-39.8 x 10-5a) If rate = k[NO]™[H2]^ what are the values of m and n?b) What is the value of k (including appropriate units)?c) What is the rate of the reaction when [NO] = 1.3 x 10-2 M and [H2] = 6.0 x 10-3 M?d) Is it possible this reaction could occur in a single elementary step? Why or why not?7. Consider the hypothetical reaction A → products. The following data was obtained over multipleexperiments by measuring the reaction half life at various initial concentrations of A.[A]ot1/20.100 M24.0 min0.150 M15.9 min0.300 M8.02 min0.400 M5.95 mina) What is the rate law for this reaction (assuming it's either zero order, first order or second order)?HINT: Try to solve part (a) without calculations!b) What is the rate constant for this reaction?8. The degradation of ethyl acetate (EA) is a first order process with t1/2 = 110 min.a) Fill in the blank: For this reaction, a graph ofvs. time will give a straight line (linear plot).b) What is the rate constant for the degradation of EA ?c) What percentage of EA will remain after 440 minutes?

Since you have posted multiple questions with multiple sub-parts, we are entitled to answer the…

6. Consider the following chemical reaction: 2 NO + 2 H2 → N2 + 2 H20 The following data was collected over three experiments: [NO] (M) 10.0 x 103 [H2] (M) Initial Rate (mol Ls) 5.0 x 105 Experiment 1 2.0 x 10-3 2 10.0 x 103 4.0 x 10-3 10.0 x 105 3 14.0 x 103 2.0 x 103 9.8 x 10-5 a) If rate = k[NO]"[(H2]^ what are the values of m and n? b) What is the value of k (including appropriate units)? c) What is the rate of the reaction when [NO] = 1.3 x 10-² M and [H2] = 6.0x 10-3 M? d) Is it possible this reaction could occur in a single elementary step? Why or why not?

6. Consider the following chemical reaction: 2 NO + 2 H2 → N2 + 2 H20 The following data was collected over three experiments: [NO] (M) 10.0 x 103 [H2] (M) Initial Rate (mol Ls) 5.0 x 105 Experiment 1 2.0 x 10-3 2 10.0 x 103 4.0 x 10-3 10.0 x 105 3 14.0 x 103 2.0 x 103 9.8 x 10-5 a) If rate = k[NO]"[(H2]^ what are the values of m and n? b) What is the value of k (including appropriate units)? c) What is the rate of the reaction when [NO] = 1.3 x 10-² M and [H2] = 6.0x 10-3 M? d) Is it possible this reaction could occur in a single elementary step? Why or why not?

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

QUESTION 1 The following data may be used for the questions that follow: NH 3(g) + BF 3(g) →F 3BNH 3(s). Initial Rate Experiment [BF3] [NH3](M) (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3. 0.200 0.100 0.0682 4 0.350 0.100 0.1193 0.175 0.100 0.0596 Based on the data in the preceding table, what is the reaction order with respect to NH 3? Zero order First order Second order Cannot be determined QUESTION 2 The following graphs can be used for the questions that follow:
The following data was collected over four different experiments. for this reaction: aA + bB → CC Experiment [A] M [B] M 1 0.200 0.200 2 0.200 0.400 3 0.400 0.200 4 0.300 0.100 The initial rate of the first reaction was 0.650 mol/L min. The second reaction was 2 times that rate, the third reaction was 8 times the rate of the first reaction, and the fourth reaction was 1.7 times the rate of the first reaction. Determine the value for the constant k. Your Answer: 2031.25
c1
A reaction AB + C → D + E has the rate equation Rate = k[AB][C]. What are the reactants in the slow step? Include a + sign between reactants with no spaces. Treat superscripts and subscripts as regular text. 2 Net
Analyze the following set of data and determine: An expression for the rate law for the reaction • A value for the rate constant with appropriate units The reaction in question is: 2A + B + 2C 1 23 EXPERIMENT INITIAL [A] (mol/L) 0.20 0.20 0.20 0.60 4 -> INITIAL [B] (mol/L) 0.10 0.30 0.10 0.30 3D INITIAL INITIAL [C] RATE (mol/L) (mol/L's) 0.10 4.0 X10-4 0.20 1.2 X 109 0.30 4.0 X 10 -4 0.40 3.6 X 10°
Using the following rate law and the experimental values given in the question figures, calculate k: Rate = k[F2][ClO2] [F2] (M) [ClO2] (M) Initial Rate (M/s) Experiment 1 0.5 0.5 0.300 Experiment 2 0.8 0.8 0.768 Experiment 3 0.5 0.8 0.480
11. The graph here shows the concentration of reagent A in a reaction. Which is the best estimate of the initial rate of the reaction? Concentration of A (moles/L) vs Time a) 625 M/s 1.000 b) 16.4 M/s 0,900 c) 0.029 M/s 0.800 0.700 d) 7.40 x 10³ M/s 0.600 0.500 0.400 0.300 0.200 0.100 0.000 60 80 0 20 40 time(s) 100 120
For the chemical reaction NO2(g) + CO(g) → NO(g) + CO2(g) The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment (mol/L) (mol/L) (mol/L.s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the rate law for the reaction? R = k [NO₂]4[CO] R = k [NO₂][CO] R = k [NO₂]²[CO] none of the answers are correct OR = K [NO₂]²
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
The balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Given the following data, estimate the rate constant of A(g) + B(g) → AB(g) (do not write the units in your answer) Experiment [A] (M) [B] (M) Rate (M/s) 1 0.400 0.200 0.8 2 0.200 0.200 0.200 0.200 0.100 0.05
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.