A chemical engineer is studying the following reaction: BF 3(aq)+ NH3(aq) → BF3NH₂(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.9. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B с compound BF3 ΝΗ, BF, NH3 BF3 NH3 BF, NH, BF3 ΝΗ, BF, NH, concentration 0.65 M 0.70 M 0.88 M 0.03 M 0.07 M 1.06 M 0.04 M 0.08 M 1.05 M expected change in concentration Ot increase O decrease ↓ Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase O decrease ↓ decrease ↓decrease Odecrease decrease decrease O decrease Odecrease O(no change) O(no change) O(no change) O(no change) O(no change) (no change) (no change) O(no change) O(no change)

A chemical engineer is studying the following reaction: BF 3(aq)+ NH3(aq) → BF3NH₂(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.9. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B с compound BF3 ΝΗ, BF, NH3 BF3 NH3 BF, NH, BF3 ΝΗ, BF, NH, concentration 0.65 M 0.70 M 0.88 M 0.03 M 0.07 M 1.06 M 0.04 M 0.08 M 1.05 M expected change in concentration Ot increase O decrease ↓ Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase O decrease ↓ decrease ↓decrease Odecrease decrease decrease O decrease Odecrease O(no change) O(no change) O(no change) O(no change) O(no change) (no change) (no change) O(no change) O(no change)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

See similar textbooks

Similar questions

12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.