3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, A,G°, is -228.57 kJ.mol', for astandard state of 1 atm. The reaction is: 2 H20 (g)→02 (g) +2H2 (g)(a) Calculate 4,G° (kJ.mol') for the above reaction.(b) Calculate the value of the equilibrium constant, K, for the above reaction.(c) Calculate the value of K, at 5 atm.

∆rG° is the Gibbs free energy of reaction which is expressed as: ∆rG°=∆fG°(products)-∆fG°(reactants)…

3.2 The standard Gibbs energy of formation of H0 at 25.0 °C, AG°, is -228.57 kJ.mol', for a standard state of 1 atm. The reaction is: 2 H20 (g)→O2 (g) +2H2 (g) (a) Calculate 4,G° (kJ.mol') for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K, at 5 atm.

3.2 The standard Gibbs energy of formation of H0 at 25.0 °C, AG°, is -228.57 kJ.mol', for a standard state of 1 atm. The reaction is: 2 H20 (g)→O2 (g) +2H2 (g) (a) Calculate 4,G° (kJ.mol') for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K, at 5 atm.

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 62QAP: Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the...

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Calculate the equilibrium constant for the following reaction at 25o C, given that change in standard Gibbs free energy (f) of O3 (g) is 163.4 kJ/mol. 2O3(g) -> 3O2(g)
Carbon may exist as diamond, graphite, and other allotropes. The standard Gibbs energy of formation of diamond is 2.900 kJ mol-1, greater than that of graphite at 298 K. Predict which of these two allotropes is the more stable at this temperature.
Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
One enzyme-catalysed reaction in a biochemical cycle has an equilibrium constant that is 8.4 times the equilibrium constant of a second reaction. If the standard Gibbs energy of the former reaction is -250 kJ mol-1, what is the standard reaction Gibbs energy of the second reaction?
An enzyme catalyzed reaction has an equilibrium constant that is 100 times the equilibrium constant of a second reaction. If the standard Gibbs energy of the former reaction is -37 kJ/mol, what is the standard reaction Gibbs energy of the second reaction? Assume the reactions take place at room temperature.
The standard Gibbs energy of formation of gaseous ozone at 25.0 ℃ ΔfGo, is162.3 kJ. mol-1, for standard state of 1 bar. The reaction is: 3O2 (g) ⇌ 2O3(g). Calculate the value of the equilibrium constant, K, for the above reaction.
The standard enthalpy of combustion of the solid glycine (the amino acid, NH2CH2COOH) is −969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1. Calculate the standard Gibbs energy of formation of glycine at 298 K. Note that the nitrogen-containing species produced on combustion is taken to be N2(g).
What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous? what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean? If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system
What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
Calculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?