(10pts) Post-Lab QuestionsUse this reaction to answer both post-lab questions.One of the reactions that is often studied in an equilibrium experiment is:NH3 (aq) + H2O (1)NH4 (aq) + OH(aq). Use this reaction to answer post-lab questions 1-3.(5pts)1. Which way would the equilibrium shift if NH4Cl was added to the solution? Briefly explain.Normal : BIUX2 X2=fx 8e=(5pts)2. What would happen to the concentration of NH4 if you added OH- to the reaction? Briefly explain.NormalBIU==fx 8TxTx

Step 1:Le Chatelier's principleLe Chatelier's principle states that if a dynamic equilibrium is…

Answered: (10pts) Post-Lab Questions Use this…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.ACP

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The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
Using Le Chatelier’s Principle Use Le Chatelier’s principle (← Sec. 12-6b) to explain why the fraction of NH3 molecules that reacts with water in a very dilute solution is larger than in a more concentrated solution.
Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of the diagrams represents the equilibrium mixture if the numerical value of the equilibrium constant is 9.0?
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Table 1: Absorbance data recorded for five 0.200 M Fe(NO:)3 solutions at 20.0 °C Beaker 0.0020 M [FESCN2+] (M) Abs. 0.00200 SCN (mL) Fe(NO3)3 (mL) 5.0 0.00 0.00 M -0.001 2 5.0 2.00 8.0 x 10-5 M 0.278 5.0 3.00 1.2 x 10-4 M 0.415 4 5.0 4.00 1.6 x 10-4 M 0.555 5.0 5.00 2.0 x 10-4 M 0.671 Part 1: y=3386x+0.0043 R^2=0.9991 Part II – Determining Concentration of an Unknown Table 2: Best-fit line and Absorbance data of unknown solution Best-fit line equation from Part I Absorbance reading of unknown 0.338 Part III – Determining the Equilibrium Constant Test tube 0.0020 M 0.00200 H20 (mL) Abs. Net Abs Fe(NO3)3 (mL) SCN-(mL) 1 3.00 0.00 7.00 0.000 2 3.00 2.00 5.00 0.119 0.119 3 3.00 3.00 4.00 0.212 0.212 4 3.00 4.00 3.00 0.265 0.265 5 3.00 5.00 2.00 0.335 0.335
Kinetics and Equilibrium Calculating an equilibrium constant from a heterogeneous equilibrium... Try Again Try again... Bis 2/5 Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. Fluoride anion and hydronium cation react to form hydrofluoric acid and water, like this: F (aq)+H3O (aq)→HF (aq) + H2O(l) At a certain temperature, a chemist finds that a 9.9 L reaction vessel containing an aqueous solution of fluoride anion, hydronium cation, hydrofluoric acid, and water at equilibrium has the following composition: compound amount F 0.146 g H₂O 0.364 g HF 4.96 g 892. g H₂O Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K 8.4 x 10 C
Activity 1: Complete Me! Direction: Complete the following table. Write your answer on a separate sheet of paper. Equilibrium Reaction Effect Keq expression Stress Equilibrium shift (encircle your answer) Forward applied (encircle your answer) Ha + Cla = | 2HCI Decreasing the pressure (increase, decrease, no change) in the number (HCIJ Keq - Backward No Shift of moles of HCl(g) (increase, decrease, no change) in the volume of Increasing Fe,O +4 Ha + heat 2 Forward Keq = the Backward 3Fe + 4H,O temperature No Shift water vapor collected of (increase, decrease, no change) the number of moles of NO 2NO + Oz 2NO + heat Forward Backward No Shift Addition (NO,P |NO]F|0,]| Keq = helium Forward H,CO» = CO2 + H,O Removal of (increase, decrease, no change) in the amount Keq - (H,CO, CO2 Backward No Shift of H,CO, (increase, decrease, no change) in amount of o, (increase, the volume of decrease, no change) in the Increasing the Forward Backward No Shift Keq= temperature the 4 NH3%g + 502 2 4NO+ 6…
ts/199084620/work Credit) | Lab: Reversible Reactions W 3) Matching. Reaction 2: Cobalt Chloride The color the COCI4+ 6H₂O Co(H₂0)6+²+4Cl 4) Choose the best answer. in the solution demonstrates that the equilibrium in this reaction is to ✓, causing a greater concentration of Co(H₂0)6+2 ions. Target due: Last Adding hydrochloric acid to the solution causes the equilibrium to shift to the CoCl2 because there is an increase in ▾ions. This gives the solution a color. Why does adding water cause a color change? O Water is a product of our original reaction, and when we added it, the concentration of the cobalt complex ion on the left side of the equation increased. Previous Sign out Next =
Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. 2 H₂S(g) + SO₂(g) = 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - Xx +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050 - x 0.025-3x 3 3 S(s) +3x 0.050 - 2x --X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + x
Write the basic equilibrium equation for (CH3)2NH. Be sure to include the proper phases for all species within the reaction. 1 U + 4 2 0₂ Reset ( H₂O 3 ) 4 5 → (CH3)2NH OH- 5 6 6 (s) 2+ 7 N H3O+ 3+ 4+ 8 9 0 ☐o (1) • H₂O 9 (g)) (aq) H Delete
When a chemical reaction is at equilibrium, the forward and reverse reactions occur at the same rate The concentrations of the different compounds in the reactions will remain constant. The relationship between the concentrations of the reactants and products is expressed as the equilibrium constant, Ke Drag each item to the appropriate bin. ▸View Available Hint(s) [0₂] Numerator Submit [H₂O]² [HC] [HCI] [Cl₂] Denominator 10₂1² [H₂O] Not used Reset Help [Cl₂1²

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