takeAssignment/takeCovalentActivity.do TripAdvisor Facebook (Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.286 mol NH,I, 8.37x10-3 M NH, and 8.37x10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.55x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI) M Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next Fmail Instructor Save and Exit

takeAssignment/takeCovalentActivity.do TripAdvisor Facebook (Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.286 mol NH,I, 8.37x10-3 M NH, and 8.37x10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.55x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI) M Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next Fmail Instructor Save and Exit

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.3: Determining An Equilibrium Constant

Problem 15.3CYU: A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent...

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12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.
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?
Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?
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?