QUESTION 18 If an elementary reaction is exothermic, then O a. the activation energy for the forward reaction is smaller than that for the reverse reaction. O b. the sum of activation energies gives the value of AH for the reaction. O c. the activation energy for the forward reaction is larger than that for the reverse reaction. O d. the activation energy for the forward reaction is negative, and for the reverse reaction, positive. O e. the activation energy for the forward reaction is positive, and for the reverse reaction, negative. QUESTION 19 Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are O a. pure liquids and gases. O b. pure solids and liquids. O C. pure solids only. O d. pure solids, liquids and gases. O e. pure liquids only.

QUESTION 18 If an elementary reaction is exothermic, then O a. the activation energy for the forward reaction is smaller than that for the reverse reaction. O b. the sum of activation energies gives the value of AH for the reaction. O c. the activation energy for the forward reaction is larger than that for the reverse reaction. O d. the activation energy for the forward reaction is negative, and for the reverse reaction, positive. O e. the activation energy for the forward reaction is positive, and for the reverse reaction, negative. QUESTION 19 Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are O a. pure liquids and gases. O b. pure solids and liquids. O C. pure solids only. O d. pure solids, liquids and gases. O e. pure liquids only.

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

The rate of reaction is halved when temperature decreases from 32 C to 25 C. What is the value of the activation energy of such a reaction? a. 63.8 kJ/mol b. -63.8 kJ/mol c. 52.9 kJ/mol c. -52.9 kJ/mol
Which of the following is/are true regarding catalysis O a. The rate constant remains the same O b. none of the above O c. All of the catalyst is consumed during the reaction O d. The activation energy is decreased
s) For a reaction, the activation energy of the forward reaction is 102 kJ and the activation energy of the reverse reaction is 120 kJ. a. What is the AH of the reaction? b. Is the reaction endothermic or exothermic? c. If a catalyst is added to the reaction, what will happen to each of the following (increase, decrease, or stay the same)? I. Activation energy of the forward reaction Activation energy of the reverse reaction AH of the reaction II. III. IV. Rate of the reaction
Page 11 ReactionThates (U State the effect of each on the rate of reaction as (1) increases, (D) decreases, or (N) no change. A. Increasing the temperature. B. Removing some of the reactants. C. Adding a catalyst! D. Placing the reaction flask in ice. E. Increasing the concentration of a reactant.
rate: k[A]^x[B]^y The rate of reaction generally increases with temperature because ____ generally increases with temperature. A. k B.[A] C. [B] D.x E.x
Consider the following mechanism: NO → N + O O + O3 → 2 O2 O2 + N → NO2 What is the role of O2? A. product only B. intermediate only C. Both intermediate and product D. reactant E. catalyst
For items 7 - 11. Select the correct answers on each item. PS. this is not graded.
250 - 200 - E (kJ) Os + NO 150 - 100 - O2 + NO2 50 - Time (seconds) a. Is the reaction endothermic or exothermic? Ans. b. What is the activation energy for the reaction? Ans. c. Assuming that the reaction is reversible, what is the value of the activation energy for the reverse reaction? Ans.
Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
Using the reaction and data in the table below answer the following series of questions. Reaction NO conc. O2 conc. Initial Rate (M/s) 1 0.500 M 0.200 M 2.2 x 10-4 2 0.250 M 0.200 M 5.6 x 10-5 3 0.250 M 0.400 M 1.1 x 10-4 *conc = concentration a. The reaction is order in regards to NO. b. The reaction is order in regards to O2.
2. What is the unit of k for each of the following type of reaction? First order reaction a. b. Second order reaction Third order reaction c.
Answer the following question using the reaction coordináte diagram shown below. 280 240 200 160 120- 80 40 Time What is the activation energy for the reverse reaction? O A. -160 kJ B. -80 kJ O C. 80 kJ D. 160 kJ tent (H) kilojoules