Consider the following reaction where K. = 1.29×102 at 600 K: COCI, (g) CO (g) + Cl2 (g) A reaction mixture was found to contain 0.135 moles of COCI, (g), 2.34×102 moles of CO (g), and 4.51×102 moles of Cl, (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following; ] 1. In order to reach equilibrium COCI2(g) must be produced . | 2. In order to reach equilibrium K. must decrease . | 3. In order to reach equilibrium CO must be produced . | 4. Qc is less than K. | 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where K. = 1.29×102 at 600 K: COCI, (g) CO (g) + Cl2 (g) A reaction mixture was found to contain 0.135 moles of COCI, (g), 2.34×102 moles of CO (g), and 4.51×102 moles of Cl, (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following; ] 1. In order to reach equilibrium COCI2(g) must be produced . | 2. In order to reach equilibrium K. must decrease . | 3. In order to reach equilibrium CO must be produced . | 4. Qc is less than K. | 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

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.
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.)
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-.
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.)
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?
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.
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?
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.
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
Predict the temperature at which the reaction in Exercise 17.67 comes to equilibrium. Consider the equation G = H TS. At some value of T, G equals zero and the reaction is at equilibrium. Set G = 0, substitute for H and S (assuming that they do not vary much with temperature) and solve for T. CH3CHO(l)+52O2(g)2CO2(g)+2H2O(l)
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?