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1. Consider the following hypothetical aqueous reaction: A(aq) – B(aq) A flask is charged with 0.200 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) Moles of A 20 0.140 40 0.100 60 0.070 80 0.200 0.050 a. Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates. b. Calculate the average rate of disappearance of A for each 20-min interval in units of M/s. c. Calculate the average rate of disappearance of A from the start of reaction to t 80 min in units of M/s. d. Between t = 0 min and t = 60 min, what is the average rate of appearance of B in units of M/s? Assume that the volume of the solution is constant.

1. Consider the following hypothetical aqueous reaction: A(aq) – B(aq) A flask is charged with 0.200 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) Moles of A 20 0.140 40 0.100 60 0.070 80 0.200 0.050 a. Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates. b. Calculate the average rate of disappearance of A for each 20-min interval in units of M/s. c. Calculate the average rate of disappearance of A from the start of reaction to t 80 min in units of M/s. d. Between t = 0 min and t = 60 min, what is the average rate of appearance of B in units of M/s? Assume that the volume of the solution is constant.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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LEARNING ACTIVITY 2 1. Consider the following hypothetical aqueous reaction: A(aq) – B(aq) A flask is charged with 0.200 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) Moles of A 20 0.140 40 0.100 60 0.070 80 0.050 0.200 a. Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates. b. Calculate the average rate of disappearance of A for each 20-min interval in units of M/s. c. Calculate the average rate of disappearance of A from the start of reaction to t = 80 min in units of M/s. d. Between t = 0 min and t = 60 min, what is the average rate of appearance of B in units of M/s? Assume that the volume of the solution is constant. 2. For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant: a. Os(g) + H2O(g) → 2 O2(g) + Hz(g) b. 4 NH3(g) + 5 Oz(g) → 4 NO(g) + 6 H;O(g) c. 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) d. CaH;NH2(g) –→ CaHe(g) + NH3(g) 3. Consider the reaction Os(g) + H2O(g) → 2 Oz(g) + H2(g). If the concentration of Os is decreasing at the rate of 0.025 M/s, what are the rates of change in the concentrations of Oz and H2?
Transcribed Image Text:LEARNING ACTIVITY 2 1. Consider the following hypothetical aqueous reaction: A(aq) – B(aq) A flask is charged with 0.200 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) Moles of A 20 0.140 40 0.100 60 0.070 80 0.050 0.200 a. Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero and that A cleanly converts to B with no intermediates. b. Calculate the average rate of disappearance of A for each 20-min interval in units of M/s. c. Calculate the average rate of disappearance of A from the start of reaction to t = 80 min in units of M/s. d. Between t = 0 min and t = 60 min, what is the average rate of appearance of B in units of M/s? Assume that the volume of the solution is constant. 2. For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant: a. Os(g) + H2O(g) → 2 O2(g) + Hz(g) b. 4 NH3(g) + 5 Oz(g) → 4 NO(g) + 6 H;O(g) c. 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) d. CaH;NH2(g) –→ CaHe(g) + NH3(g) 3. Consider the reaction Os(g) + H2O(g) → 2 Oz(g) + H2(g). If the concentration of Os is decreasing at the rate of 0.025 M/s, what are the rates of change in the concentrations of Oz and H2?
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