8. The rate of a reaction is doubled by a certain rise in temperature just when the reaction begins, i.e. ¤ = 0. Will the rate be also doubled for a = 0.5? 9. There is 60% reduction in the value of the rate constant of a reaction when the reaction temperature decreases from 60 to 40 °C. What is the activation energy

8. The rate of a reaction is doubled by a certain rise in temperature just when the reaction begins, i.e. ¤ = 0. Will the rate be also doubled for a = 0.5? 9. There is 60% reduction in the value of the rate constant of a reaction when the reaction temperature decreases from 60 to 40 °C. What is the activation energy

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

Don't Hand writing in solution.
Suppose you could measure the rate constants for both the forward and reverse reactionsof the process in Figure 14.16. In which direction would the rate constant be larger?
= ○ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +C1(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. 1 Write an expression that gives the equilibrium concentration of CFC1, in terms of k₁, k₁, and the equilibrium concentrations of CFC13 and C1. 1' [CFC₁₂] = 0 √6 X 5 0/5
It was determined experimentally that the reaction rate remained the same when the concentration of A was doubled in the following reaction: A + B → CThe reaction is ________ order in A.
5. Data for the reaction of ammonium and nitrite ions in water at 25°C follows. Determine the rate law for this reaction. Rate ( M/sec) [NO,] 0.01 NH,"] 0.2 5.4 X 10 - 10.8 X 10 21.5 X 10 32.2 X 10-7 0.02 0.2 0.04 0.2 0.06 0.2 0.2 0.02 10.8 X 107 0.2 0.04 21.6 X 10-7 0.2 0.06 32.4 X 10-7 0.2 0.08 43.3 X 10-7
A certain reaction has an activation energy of 44.26 kJ/mol. At what Kelvin temperature will the reaction proceed 7.50 times faster than it did at 365 K?
Part A: What is the value of the activation energy of the uncatalyzed reaction? Part B: What is the value of the enthalpy change of the uncatalyzed reaction? Part C: What is the value of the activation energy of the uncatalyzed reaction in reverse? Part D: What is the value of the enthalpy change of the uncatalyzed reaction in reverse?
Given the same reactant concentrations, the below reaction at 257. °C is 94.6 times as fast as the same reaction at 163. °C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant. Round your answer to 2 significant digits. co(g) + Cl₂(g) - COCL, (g) Note: Reference the Fundamental constants table for additional information. E₁ - 1 kJ mol x10 X
10. Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO2(g) [NO] (M) [02] (M) Initial Rate (Ms ¹) A. Rate 57 M¹s¹ [NO][O₂] B. Rate = 3.8 M-1/2 5-1[NO][O₂] 1/2 C. Rate = 3.1 × 105 M¯³s¯¹[NO]²[O₂]² D. Rate = 1.7 × 10³ M²s¯¹[NO]²[02] E. Rate = 9.4 × 10³ M²s¯¹[NO][O₂]² -2 0.030 0.0055 8.55 x 10-3 0.030 0.0110 1.71 × 10°² -2 0.060 0.0055 3.42 × 10-2
Determine the rate law and the value of k for the following reaction using the data provided. CO(g) + Cl2(g) COC(g) [CO]; (M) [Cl2]; initial rate (M 1s1) 0.25 0.40 0.696 0.25 0.80 1.97 0.50 0.80 3.94 O Rate = 11 Ms [CO][Cl2]} Rate 36 M-1.8 5-1 [CO][Cl2]²8 || O Rate = 17 M-²s-' [CO][Cl2]² -1 O Rate = 4.4 MT|CO][Cl½]? M7s- [CO][Cl2]? S -3 O Rate = 18 M5-|co){{Cl2]} S
13. A reaction A+B+C → D follows the mechanismA  B   C A B  C   Din which the first step remains essentially in equilibrium. Show that the dependence of rate on temperature is given byk  Ae(Ea H )/RTwhere H is the enthalpy change for the first reaction.
At a given temperature, the elementary reaction A↽−−⇀B,A↽−−⇀B, in the forward direction, is first order in AA with a rate constant of 0.0220 s−1.0.0220 s−1. The reverse reaction is first order in BB and the rate constant is 0.0840 s−1.0.0840 s−1. What is the value of the equilibrium constant for the reaction A↽−−⇀BA↽−−⇀B at this temperature? ?=K= What is the value of the equilibrium constant for the reaction B↽−−⇀AB↽−−⇀A at this temperature? ?=