Consider the decomposition of a metal oxide to its elements, where M represents a Substance AG (kJ/mol) generic metal. M,0(s) -6.40 M(s) M,O(s) = 2 M(s) +0,(g) 0,(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? AG¡xn kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = What is the equilibrium pressure of O,(g) over M(s) at 298 K?

Consider the decomposition of a metal oxide to its elements, where M represents a Substance AG (kJ/mol) generic metal. M,0(s) -6.40 M(s) M,O(s) = 2 M(s) +0,(g) 0,(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? AG¡xn kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = What is the equilibrium pressure of O,(g) over M(s) at 298 K?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 83QAP

See similar textbooks

Similar questions

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.)
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.
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
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.
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-.
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
Given the following data at 25C 2NO(g)N2(g)+O2(g)K=1 10 30 2NO(g)+Br2(g)2NOBr(g)K=8 101 Calculate K for the formation of one mole of NOBr from its elements in the gaseous state.
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
Use data given in Tables 6.2 and 18.1 to obtain the value of Kp at 1000C for the reaction C(graphite)+CO2(g)2CO(g) Carbon monoxide is known to form during combustion of carbon at high temperatures. Do the data agree with this? Explain.
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?
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?