The activation energy for a first-order reaction is 150 kJ/mol. The value of the rate constant (k) is 5.2 × 10-12 s-1 at 45°C. What is the value of k at 227°C? 1.5 x 1011 S-1 4.7 x 10-35-1 6.7 x 10-22 S-1 1.1 x 1029 S-1 2.1 x 1013 S-1

The activation energy for a first-order reaction is 150 kJ/mol. The value of the rate constant (k) is 5.2 × 10-12 s-1 at 45°C. What is the value of k at 227°C? 1.5 x 1011 S-1 4.7 x 10-35-1 6.7 x 10-22 S-1 1.1 x 1029 S-1 2.1 x 1013 S-1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 31QRT

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The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1) [B](mol L ’) Rate = A(C]/Af (mol L-1 s-1) 0.127 0.15 0.033 0.127 0.30 0.132 0.255 0.15 0.066 Determine the reaction order for each reactant and the value of the rate constant.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (a) Rate = k [X][Y][Zl, (b) Rate = k [X]-[Y]1/2[Z], (c) Rate = k [X]L5[Y]-1, (d) Rate = k [X]/[Y]2
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.
Based on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.
The data in the table are for the reaction of NO and O2 at 660 K. NO(g) + O2(g) NO2(g) (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant. (d) Calculate the rate (in mol/L s) at the instant when [NO] = 0.015 mol/L and [O2] = 0.0050 mol/L. (e) At the instant when NO is reacting at the rate 1.0 104 mol/L s, what is the rate at which O2 is reacting and NO2 is forming?
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.
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?

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