Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) ▾ Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. 1 A/N₂0] Rate At O Rate = Ⓒ Rate = ✓ Correct Part B = =- At 1 AN₂ Rate = -10 = N -- At At Submit Previous Answers Rate = Submit Part C A[N₂0 At AIN₂0] At AN₂0] At Submit =11202 N140, == 1 A[N₂] 2 At In the first 13.0s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE] ΑΣΦ Request Answer A(O₂) At = Request Answer At 14/01 At A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O)/At? Express your answer using two significant figures. 195] ΑΣΦΑ ? → C M.s1 ? M-81

Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) ▾ Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. 1 A/N₂0] Rate At O Rate = Ⓒ Rate = ✓ Correct Part B = =- At 1 AN₂ Rate = -10 = N -- At At Submit Previous Answers Rate = Submit Part C A[N₂0 At AIN₂0] At AN₂0] At Submit =11202 N140, == 1 A[N₂] 2 At In the first 13.0s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE] ΑΣΦ Request Answer A(O₂) At = Request Answer At 14/01 At A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O)/At? Express your answer using two significant figures. 195] ΑΣΦΑ ? → C M.s1 ? M-81

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
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.
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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.
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
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Why does a catalyst increase the rate of a reaction? What is the difference between a homogeneous catalyst and a heterogeneous catalyst? Would a given reaction necessarily have the same rate law for both a catalyzed and an uncatalyzed pathway? Explain.