7. Which of the following statements is true for a reaction with the equilibrium constant K,= 7.6 x 10? Kpis the pressured based equilibrium constant; AG° is the Gibbs energy change of the reaction at the standard state condition. a) AG°>0 and the reaction is reactant favored b) AG°>0 and the reaction is product favored c) AG° <0 and the reaction is product favored d) AG<0 and the reaction is reactant favored e) none of the above

7. Which of the following statements is true for a reaction with the equilibrium constant K,= 7.6 x 10? Kpis the pressured based equilibrium constant; AG° is the Gibbs energy change of the reaction at the standard state condition. a) AG°>0 and the reaction is reactant favored b) AG°>0 and the reaction is product favored c) AG° <0 and the reaction is product favored d) AG<0 and the reaction is reactant favored e) none of the above

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

Section12.5: Using Equilibrium Constants

Problem 12.7CE

See similar textbooks

Similar questions

Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
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.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)
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.)
5.11. Determine the numerical value of Q for the reaction conditions indicated.