a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq.    A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species.   You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?

Q: Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘C using the table of thermodynamic…

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Q: The value of ΔE in kJ, for a system that does 213 kJ of work on its surroundings and loses 79 kJ of…

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Q: The standard Gibbs free energy change at 100oC is 18.8 kJ/mol for the solubility equilibrium:…

A: Given ReactionLi3PO4 (s) → 3 Li+ (aq)   +  PO43-(aq)∆Grxn0 = 18.8 kJ/mole = 18800 J/moleT = 100°C =…

Q: Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Refer to the AG°{…

A: The  question is based on concept of chemical thermodynamics. we have to calculate Gibbs free energy…

Q: Aa.46. We start with a pure sample of A(g). The following equilibrium is established: 2 A(g) B(g)…

A: Here we have  to determine standard Gibbs free enery for the  following given reactions.

Q: The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn…

A: We have given that ∆G° = 1.92×105 J/mole T  = 298 K ∆H° = 243.5 kJ /mole ∆S° = 170 J/mole = 0.170…

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.