Gibbs Free Energy

Related Topics

Wize University Chemistry Textbook > Thermodynamics Part 2: (2nd Law-entropy, 3rd Law, Gibbs Free Energy, Spontaneity)

Connecting Gibbs Free Energy and Equilibrium

7 Activities

Determine the value of K for these reactions

a.

b.

c.

I don't know

More Connecting Gibbs Free Energy and Equilibrium Questions:

Use the following reactions to answer the questions below
Cu(s)+2Ag+(aq)⇌Cu2+(aq)+2Ag(s)Cu(s)+2Ag^+(aq)⇌Cu^{2+}(aq)+2Ag(s)Cu(s)+2Ag+(aq)⇌Cu2+(aq)+2Ag(s)    Spontaneous; E = 0.46 V 
Cu(s)+Pb2+(aq)⇌Cu2+(aq)+Pb(s)Cu(s)+Pb^{2+}(aq)⇌Cu^{2+}(aq)+Pb(s)Cu(s)+Pb2+(aq)⇌Cu2+(aq)+Pb(s)       Non-Spontaneous; E = -0.47 V

For a reaction with a negative ΔGo value, which of the following statements is/are FALSE?
1. The equilibrium constant K is greater than one.
2. The reaction is spontaneous when all the reactants and products are in their standard states.

Gibbs free Energy: Equilibrium

At 699 K, Δ\DeltaΔGo = -23.25 kJ for the reaction H2 (g) + I2 (g) ⇌ 2 HI (g). Calculate Δ\DeltaΔG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product HI is at 1.00 atm
pressure.

Thermodynamics

The Solubility Constant for AgI(s) at 25oC is 8.3x10-17. What is ΔG(rxn) given that the current concentrations of ions are: [Ag+]=9.1x10-9 & [I-]=9.1x10-9

1)Write the variables we know/trying to solve for
2) Out of the different equations for deltaG, which one should we use?

Gibbs Free Energy: Formation

The value of ΔGo for the following reaction is -2745 kJ. Use this value and the information on the Data Sheet to calculate the standard free energy of formation, ΔGfo of C4H10 (g) in kJ/mol.
C4H10 (g) + 13/2 O2 (g) →\rightarrow→ 4 CO2 (g) + 5 H2O (l)
ΔGfo (CO2(g)) = -394.4 kJ/mol             ΔGfo (H2O(l)) = -237.13 kJ/mol