What is the equilibrium constant for a reaction whose AG 165 kJ/mol at 262 K?

Calcualte the change in Gibbs free energy (AG°) for the reaction below given the change in enthalpy (AH°) is CO (g) + H,O (g) – CO2 (g) + H2 (B) DH° = -41.2 kJ and Ds° = -135 J/mol K at 298 K -0.97 kļ/mol a 40188.8 kļ/mol -81.43 kJ/mol -0.77 kļ/mol

Determine the equilibrium constant for a reaction at 200 K if AG =26.2 kJ/mol. (R = 8.314 J/mol · K)

Use the following information to calculate the standard free energy change (AG°) and equilibrium constant (K) for the following system: CaCO3(s) = CaO(s) + CO2(g) T= 900.0 °C AH;° values (kJ/mol): CaO(s) = -634.9, CO2(g) = -393.51, CaCO3(s) =–1220.0 %3D S° values (J/mol K): CaO(s) = 110.0, CO2(g) = 213.8, CACO3(s) = 38.1 %3D %3D %3D

Complete and balance the following reactions - assume they all go a. solid potassium carbonate plus heatb. solid ferric chlorate plus heatc. solid sodium chromate tetrahydrate plus heat

5. Reaction Enthalpy. balance and calculate AH for the following chemical equations. AH (kJ/mol): HCN = 130.5, Ca3(PO4)2=-4120.8, H3PO4-1288, SiCl₁=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl=-167.16 d) Mg(s) + H₂0(g) 0 Mg(OH)2(s)

Using the values in Appendix F, calculate the standard free energy change for the following reaction at 25 °C. 2Ag*(aq)+Fe(s)=2Ag(s)+Fe?*(aq) O-558.01 kJ/mol 89.234 kJ/mol O-240.556 kJ/mol O 121.036 kJ/mol

What is the value of the equilibrium constant for the following reaction at 25C with a delta Grxn = -6.38 kJ?  H2(g) + Cl2(g) <-> 2HCl(g)

What is the equilibrium constant for a reaction at 25oC. The value of delta G is -47.2 kJ/mol.

Determine the value of K for a reaction where AG° = -29.62 kJ/mol at 298 K. K =