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CHEM107_Exam4_Study Guide

# CHEM107_Exam4_Study Guide - Texas A M University Department...

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Texas A & M University Department of Chemistry CHEM107 Spring 2011 Instructor: Masud Monwar, Ph.D. Study Guide for Exam 4 Posted on: 26 th April, 2011 Chapter 11: Chemical Kinetics 1. a. Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. i) 2 O 3 (g) 3 O 2 (g) ii) 2HOF(g) 2HF(g) + O 2 (g) b. In reaction a(i), the rate of formation of O 2 is 1.5 × 10 -3 mol/L.s. What is the rate of decomposition of O 3 ? 2. a. Using the rate equation “Rate = k [A] 2 [B],” define the order of the reaction with respect to A and B. What is the total order of the reaction? b. The reaction between ozone and nitrogen dioxide at 231 K is first order in both the [NO 2 ] and [O 3 ]. 2NO 2 (g) + O 3 (g) N 2 O 5 (s) + O 2 (g) i) Write the rate equation for the reaction. ii) If the concentration of NO 2 is tripled, what is the change in the reaction rate? iii) What is the effect on reaction rate if the concentration of O 3 is halved? c. The data in the table are for the reaction of NO and O 2 at 660 K. 2NO(g) + O 2 (g) 2NO 2 (g) Reactant concentration (mol/L) Rate of disappearance of NO (mol/L.s) [NO] [O 2 ] 0.010 0.010 2.5  10 -5 0.020 0.010 1.0  10 -4 0.010 0.020 5.0  10 -5 i) Determine the order of the reaction for each reactant. ii) Write the rate equation for the reaction. Continued to page 2 iii) Calculate the rate constant.

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iv) Calculate the rate(in mol/L.s) at the instant when [NO] =0.015 mol/L and [O 2 ]=0.0050 mol/L. v) At the instant when NO is reacting at the rate 1.0 × 10 -4 mol/L.s, what is the rate at which O 2 is reacting and NO 2 is forming? d. A reaction has the following experimental rate equation: Rate = k[A] 2 [B]. If the concentration of A is doubled and the concentration of B is halved, what happens to the reaction rate? 3. Data for the reaction 2NO(g) + O 2 (g) ------- 2NO 2 (g) are given in the table. Experiment Concentration (mol/L) Initial rate (mol/L.h) [NO] [O 2 ] 1 3.6  10 -4 5.2  10 -3 3.4  10 -8 2 3.6  10 -4 1.04  10 -2 6.8  10 -8 3 1.8  10 -4 1.04  10 -2 1.7  10 -8 4 1.8  10 -4 5.2  10 -3 ? a) What is the rate law for this reaction? b) What is the rate constant for the reaction? c) What is the initial rate of the reaction in experiment 4? 4. a) The rate equation for the hydrolysis of sucrose to fructose and glucose C 12 H 22 O 11 (aq) + H 2 O(l) ------------- 2C 6 H 12 O 6 (aq) Is “- [sucrose]/ t = k [C 12 H 22 O 11 ].” After 2.57 h at 27 ° C, the sucrose concentration decreased from 0.0146 M to 0.0132 M. Find the rate constant. b) The decomposition of SO 2 Cl 2 is a first-order reaction: SO 2 Cl 2 (g) ------- SO 2 (g) + Cl 2 (g) The rate constant for the reaction is 2.8 × 10 -3 min -1 at 600K. If the initial concentration of SO 2 Cl 2 is 1.24 × 10 -3 mol/L, how long will it take for the concentration to drop to 0.31 × 10 -3 mol/L? 5. a) The rate equation for the decomposition of N 2 O 5 (giving NO 2 and O 2 ) is “- [N 2 O 5 ]/ t = k [N 2 O 5 ].” The value of k is 5.0 × 10 -4 s -1 for the reaction at a particular temperature.
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CHEM107_Exam4_Study Guide - Texas A M University Department...

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