Calculate `DeltaG^(@)` (kJ/mol) at `127^(@)C` for a reaction with `K_("equilibrium")=10^(5)` :

The value of DeltaG^(@) for a reaction is 7.97 KJ//"mole" . Its equilibrium constant K_(c) at 298K is 4 xx 10^(-x) What is x?

Calculate DeltaG and DeltaG^(@) for the reaction: A + B iff C+ D at 27^(@)C for which K = 10^(2) .

The K_(sp) of calcium flouride is 3.2xx10^(-11) . Calculate the DeltaG^(@) (in KJ.mol^(-1) ) for the dissolving of solid calcium fluoride at 25^(@) C.

Calculate E_(cell)^(@) and DeltaG^(@) for the following reaction at 25^(@)C . A^(2+)+B^(+) to A^(3+)+B (Given K_(c)=10^(10) , 1F=96500" C mol"^(-1) )

At 300 K, A hArr" Product"DeltaG_(T)^(@)=-"200 kJ mol"^(-1) BhArr" Product "DeltaG_(T)^(@)=-"50 kJ mol"^(-1) Thus, the ratio of equilibrium constant at 300 K

At 300 K, A hArr" Product"DeltaG_(T)^(@)=-"200 kJ mol"^(-1) BhArr" Product "DeltaG_(T)^(@)=-"50 kJ mol"^(-1) Thus, the ratio of equilibrium constant at 300 K

Molar heat capacities at constant pressure for A, B and C are 3, 1.5 and 2 J/K mol. The enthalpy of reaction and entropy of reaction, A + B rarr 3C are 20 kJ/mol and 20 J/K mol at 300 K. Calculate DeltaG (in kJ / mol) for the reaction, (1)/(2)A+Brarr(3)/(2)C

Molar heat capacities at constant pressure for A, B and C are 3, 1.5 and 2 J/K mol. The enthalpy of reaction and entropy of reaction, A +2 B rarr 3C are 20 kJ/mol and 20 J/K mol at 300 K. Calculate DeltaG (in kJ / mol) for the reaction, (1)/(2)A+Brarr(3)/(2)C

Molar heat capacities at constant pressure for A, B and C are 3, 1.5 and 2 J/K mol. The enthalpy of reaction and entropy of reaction, A + B rarr 3C are 20 kJ/mol and 20 J/K mol at 300 K. Calculate DeltaG (in kJ / mol) for the reaction, (1)/(2)A+Brarr(3)/(2)C