Project #80960 - CHM 115 Chapter 12 Practice Quiz

Chapter 12 Practice Quiz

Name ___________   Section Time __________ AM/PM

Directions: Please submit all work and answers on a separate piece of paper either through LC or in class on the day it is due. You will have 30 minutes to complete the in-class quiz, which will be 15 multiple-choice questions. You will be able to write on the quiz and will be provided the following equations.  

 [A]t = -kt + [A]0            ln [A]t = -kt + ln [A]0                   t1/2 = 0.693 / k              t1/2 = [A]0 / 2k              t1/2 = 1/ k[A]0

 

 

R = 8.31 J/K-mol

 

1.     Compare and contrast the various factors that impact the rate of a reaction and the rate constant for a reaction.

 

2.     Compare the plots for first order, zero order, and second order reactions.

 

3.     For each of the following rate expressions, indicate the impact on the initial rate for each scenario.              

Rate Law

Double [A]

Double [B]

Double [A] and [B]

Triple [B]

rate = k[A][B]

 

 

 

 

rate = k[A]2[B]

 

 

 

 

rate = k[A][B]2

 

 

 

 

 

4.         Draw an energy diagram for a reaction with an activation energy of 167 kJ/mol, and DE of +28 kJ/mol.
            Label Ea,
DE, Products, Reactants, Intermediate/Transition State. Explain what makes the reaction either
            endothermic or exothermic and how this differs from the reverse reaction.

 

5.         For the energy diagram above, draw a line showing the reaction if a catalyst were involved and explain
            what a catalyst is and does.

 

6.         Determine the activation energy for a reaction with a rate constant of 3.52x10-7 L/mol∙ s at 555K, and
            9.5 x 10-5 L/mol∙s at 645K.

 

7.         If the average rate of disappearance of nitrogen gas in the reaction 2N2 (g) à 4NO2 (g) + O2 (g) was
            found to be 3.7 x 10–5 M /s. Determine the rate of appearance of NO2

 

8.         For the following reaction and experimental data provided:                 Initial [A]    Initial [B]        rate (M/s)
            2A + B
àproducts, determine the order of the reaction with       0.130           0.230                0.400
            respect to A, the order of the reaction with respect to B, and       0.260           0.230                1.60
            the overall order of the reaction.                                                    0.130            0.460              12.8                         

9.         For the above reaction, determine the value of the rate constant and be sure to include units.

 

Use the following data and first-order reaction information for questions 10-13.                 Aà B

11.       What is the rate constant for this decomposition?                                          time (sec)         [A] (M)     

12.       What was the initial concentration of [A]?                                                     3.0                   0.86

13.       What would the concentration be after 5.0 seconds?                                     6.0                   0.61

10.       What is the half-life for this reaction?                                                            9.0                   0.43

 

14.       The reaction A à products is first order. If the concentration of A decreases from 0.050 M to 0.025 M
            after 14 minutes, determine the rate constant of the reaction.

 

15.       Determine the rate law based on the proposed mechanism below.     

                                                            Step 1  A + B E                  fast 

 

                                                            Step 2  E + A ® C + D          slow

Subject Science
Due By (Pacific Time) 09/04/2015 11:59 pm
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