Consider the following reaction where K, = 1.29×10 2 at 600 K:COCI2 (g) co (g) + Cl2 (g)A reaction mixture was found to contain 0.113 moles of COCI, (g), 4.94×10 2 moles of CO (g), and 3.74x10 2 moles of Cl, (g), in a 1.00 liter container.Indicate True (I) or False (E) for each of the following:1. In order to reach equilibrium COCI2(g) must be consumedv 2. In order to reach equilibrium Kc must decrease.v 3. In order to reach equilibrium CO must be produced .|v 4. Qc is greater than Kc.v 5. The reaction is at equilibrium. No further reaction will occur.

Given-> Kc = 1.29 × 10-2 Mole of COCl2= 0.113 mole Mole of CO = 4.94 × 10-2 mole Mole of Cl2 =…

Consider the following reaction where K. = 1.29x10-2 at 600 K: COCI2 (g) co (g) + Cl2 (g) A reaction mixture was found to contain 0.113 moles of COCI, (g), 4.94x10-2 moles of CO (g), and 3.74x10 2 moles of Cl (g), in a 1.00 liter container. Indicate True (I) or False (F)_for each of the following: v 1. In order to reach equilibrium COCI2(g) must be consumed . v 2. In order to reach equilibrium K. must decrease . v 3. In order to reach equilibrium CO must be produced v 4. Qç is greater than Kc. v 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where K. = 1.29x10-2 at 600 K: COCI2 (g) co (g) + Cl2 (g) A reaction mixture was found to contain 0.113 moles of COCI, (g), 4.94x10-2 moles of CO (g), and 3.74x10 2 moles of Cl (g), in a 1.00 liter container. Indicate True (I) or False (F)_for each of the following: v 1. In order to reach equilibrium COCI2(g) must be consumed . v 2. In order to reach equilibrium K. must decrease . v 3. In order to reach equilibrium CO must be produced v 4. Qç is greater than Kc. v 5. The reaction is at equilibrium. No further reaction will occur.

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 61QRT

See similar textbooks

Similar questions

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?
If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)
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?
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g) at 25 C. {Vapor pressure was described in the previous Chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
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 reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.