`CO_((g))+1/2 O_(2) (g) rarr CO_(2(g))`
`DeltaH=-67.37` K.cal at `25^(@)C` the change in entropy accompanying process is `-20.7` cal.`deg^(-1) mol^(-1)` then at `25^(@)C` the change in free energy is

Heat of reaction for, CO(g) 1/2 O_(2)(g) rarr CO_(2)(g) at constant V is -67.71 kcal at 17^(@)C . The heat of reaction at constant P at 17^(@)C

CH_(4(g)) + 2O_(2(g)) rarr CO_(2(g)) + 2H_2O_((l)) DeltaH = -200 K.cal , now DeltaE Cal, now DeltaE for the same process at 300 K (in K.Cal)

Heat of reaction for, CO(g)+1//2O_(2)(g)rarr CO_(2)(g) at constant V is -67.71 K cal at 17^(@)C . The heat of reaction at constant P at 17^(@)C is :-

Heat of reaction for, CO(g)+1//2O_(2)(g)rarr CO_(2)(g) at constant V is -67.71 K cal at 17^(@)C . The heat of reaction at constant P at 17^(@)C is :-

Show that the reaction CO(g) +(1//2)O_(2)(g) rarr CO_(2)(g) at 300K is spontaneous and exothermic, when the standard entropy change is -0.094 k J mol^(-1) K^(-1) . The standard Gibbs free energies of formation for CO_(2) and CO are -394.4 and -137.2kJ mol^(-1) , respectively.

Show that the reaction CO(g) +(1//2)O_(2)(g) rarr CO_(2)(g) at 300K is spontaneous and exothermic, when the standard entropy change is -0.094 k J mol^(-1) K^(-1) . The standard Gibbs free energies of formation for CO_(2) and CO are -394.4 and -137.2kJ mol^(-1) , respectively.

C(s)+O_(2)(g)rarr CO_(2)(g)+94.0 K cal. CO(g)+(1)/(2)O_(2)(g)rarr CO_(2)(g), Delta H=-67.7 K cal. From the above reactions find how much heat (Kcal "mole"^(-1) )would be produced in the following reaction : C(s)+(1)/(2)O_(2)(g)rarr CO(g)

C(s)+O_(2)(g)rarr CO_(2)(g)+94.0 K cal. CO(g)+(1)/(2)O_(2)(g)rarr CO_(2)(g), Delta H=-67.7 K cal. From the above reactions find how much heat (Kcal "mole"^(-1) )would be produced in the following reaction : C(s)+(1)/(2)O_(2)(g)rarr CO(g)