• Part B Now, calculate the A:G for the same reaction, based on the Standard Gibbs Energies of formation: ArG"NO= 87.6 kJ - mol ArG'N;O4 = 90.8 kJ .- mot 4,G" = -75.4 kJ - mol Previous Answere Completed Part C Using two very different method to solve for A:G, your answers from part A and part B will be the same. Why? The reaction is spontaneous under all conditions O Gibbs Energy is a state function O Gibbs Energy is independent of temperature O The reaction is at equilibrium under standard conditions

• Part B Now, calculate the A:G for the same reaction, based on the Standard Gibbs Energies of formation: ArG"NO= 87.6 kJ - mol ArG'N;O4 = 90.8 kJ .- mot 4,G" = -75.4 kJ - mol Previous Answere Completed Part C Using two very different method to solve for A:G, your answers from part A and part B will be the same. Why? The reaction is spontaneous under all conditions O Gibbs Energy is a state function O Gibbs Energy is independent of temperature O The reaction is at equilibrium under standard conditions

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...

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