Directions: Write the letter of the word or phrase that best completes the statement or answers the question on the space provided. I. first order J. reaction order A. catalysts B. concentration C. rate law D. surface area E. temperature F. rate of reaction G. reactivity H. reactants 1. It refers to the amount of substance per unit volume. 2. Some reactions are slow and some are fast. 3. It tells the concentration dependence of one reactant in a reaction. 4. It is characterized as the tendency of a material to undergo a chemical reaction. 5. It shows the relationship between concentrations of reactants and reaction rate. 6. It describes the powers of the concentration factors in the rate equation. 7. It is a property of a material which increases as particle size decreases. 8. These are substances that go away with time in a reaction. 9. It increases the kinetic energy present in a material. 10. These are materials that do not change their amount throughout the chemical reaction.

Directions: Write the letter of the word or phrase that best completes the statement or answers the question on the space provided. I. first order J. reaction order A. catalysts B. concentration C. rate law D. surface area E. temperature F. rate of reaction G. reactivity H. reactants 1. It refers to the amount of substance per unit volume. 2. Some reactions are slow and some are fast. 3. It tells the concentration dependence of one reactant in a reaction. 4. It is characterized as the tendency of a material to undergo a chemical reaction. 5. It shows the relationship between concentrations of reactants and reaction rate. 6. It describes the powers of the concentration factors in the rate equation. 7. It is a property of a material which increases as particle size decreases. 8. These are substances that go away with time in a reaction. 9. It increases the kinetic energy present in a material. 10. These are materials that do not change their amount throughout the chemical reaction.

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...

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14. Why does the rate of the reaction decrease over time? A. Exothermic reactions lose heat which cools the reaction which decreases the reaction rate. B. As the reaction proceeds, the concentration of the products results in fewer collisions. C. As the reaction proceeds, a decrease in the concentration of reactants results in fewer successful collisions. D. Not all molecules will react and some choose to stay in their present form. E. none of the above
Answer question numbers 10, 11 and 12
10. The rate of reaction measures how fast a reactant is consumed or a product is formed. The rate is expressed as the ratio of the change in the concentration to elapsed time. A. Only the first statement is correct. B. Only the second statement is correct. C. Both statements are correct. D. Both statements are incorrect.
a. b. C. d. e. 1. If for the reaction a b d e aX → by → 9 the rate law is determined to be r=[X]¹[Y]º the order of the reaction is 0 increasing the concentration of Y will have no effect on the rate increasing the concentration of X will have no effect on the rate increasing the concentration of Y will increase the rate of the reaction there is no way to determine the value of k 9 then
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16. A reaction mechanism proposes three step reactions for the overall reaction and the energy diagram shows three activated states. From the proposed mechanism and energy diagram how many reaction intermediates are expected to form?A. 3 B. none C. 1 D. 2 E. 4
QUESTION 7 Match the part of the rate law with the correct term. 2 NO(g) + Cl2(g) --> 2 NOCI(g) 2. rate 3.0 mol2*s A 3.0 mol2*s A. Y rate constant vorder of reaction with respect to NO vorder of reaction with respect to Cl2 В. 1 C. 2 overall reaction order D. 3 QUESTION 8 2.
d.The simplifying assumption that the change in concentration of the reactants is SMALL (and therefore negligible to the calculation) compared to the initial concentration of the reactants. Is this assumption justified in this reaction and these conditions? Do a little math to prove your point.