CHE 221-222 Lab.. • Saved -A KatlynFileHome Insert Draw Design Layout References Mailings Review View HelpBe careful-files from the Internet can contain viruses. Unlessyou need to edit, it's safer to stay in Protected View.PROTECTED VIEWEnable Editing1. Use Le Chatelier's Principle to answer the questions about the following reversible reaction:N204 (g) = 2N02 (g)a. If the concentration of N2O4 is increased, what will happen to the equilibrium of thereaction? Will it shift in the reverse direction to favor the formation of N2O4, will itshift forward to favor the formation of NO2, or will it stay the same?b. You are observing this reaction in a closed container. What will happen to theequilibrium if you increase the pressure inside the container? Will it shift in thereverse direction to favor the formation of N2O4, will it shift forward to favor theformation of NO2, or will it stay the same?2. The reaction you will be manipulating in this experiment is:[Co(H20)6]2+ (aq) + 4Cl (aq) = [CoCl4]² (aq) + 6H2O (I)[Co(H20)6]2+ is a metal complex that forms a pink solution when mixed with water, while asolution of [CoCl4]2- has a blue color. You will monitor the reaction according to the color ofthe reaction mixture.a. Write an expression for the K of this reaction. Note that this is a heterogeneousreaction.b. Read the instructions for Part A of week 1. What "stress" are you placing on thereaction as you compare test tubes "a" through "e"? Would you expect this stress toshift the reaction in the forward direction or in the reverse?C. Read the instructions for Part B of week 1. What "stress" are you placing on thereaction as you compare test tubes "f" through "j"? Would you expect this stress toshift the reaction in the forward direction or in the reverse?d. In Part C of week 1, you will observe how temperature affects equilibrium. If areaction is endothermic, how would you expect increasing temperature to shift theequilibrium? Wwhat if a reaction is exothermic?3. Review Beer's Law. You have a 2.5 M aqueous sample of a metal ion, which has anabsorbance of 0.75 at 660 nm. An unknown solution of the same metal ion, on the same dayand on the same spectrophotometer, has a measured absorbance of 0.59. What is theconcentration of metal ion in the unknown solution?Page 115 of 1552 of 37707 wordsD Focus目97%

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- Use Le Chatelier's Principle to answer the questions about the following reversible reaction: 204 (g) = 2NO2 (g) a. If the concentration of N204 is increased, what will happen to the equilibrium of the reaction? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same? b. You are observing this reaction in a closed container. What will happen to the equilibrium if you increase the pressure inside the container? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same?

- Use Le Chatelier's Principle to answer the questions about the following reversible reaction: 204 (g) = 2NO2 (g) a. If the concentration of N204 is increased, what will happen to the equilibrium of the reaction? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same? b. You are observing this reaction in a closed container. What will happen to the equilibrium if you increase the pressure inside the container? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same?

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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4) For the reaction shown below, at a particular time, the following concentrations are obtained: [N2O4] = 2.00 M, [NO2] = 0.20 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? N2O4 (g) « 2 NO2 (g)Kc = 0.200
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