Consider the following reaction where KcNH4Cl(s) ⇒ NH3(g) + HCl(g)A reaction mixture was found to contain 0.0531 moles of NH4Cl(s), 0.00147 moles of NH3(g), and 0.00226 moles of HC1(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Q, equals=Submit Answer-65.10 x 107 at 548 K.The reactionO must run in the forward direction to reach equilibrium.O must run in the reverse direction to reach equilibrium.O is at equilibrium.Use the References to access important values it needed for this question.Retry Entire Group 9 more group attempts remaining

Consider the following reaction where Ke = 5.10 x 10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction mixture was found to contain 0.0531 moles of NH4Cl(s), 0.00147 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium. Submit Answer Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining

Consider the following reaction where Ke = 5.10 x 10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction mixture was found to contain 0.0531 moles of NH4Cl(s), 0.00147 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium. Submit Answer Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 3ALQ: For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each...

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Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
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.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
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.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.