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[" 2."CO((g))+(1)/(2)O(2)(g)rarr CO(2(g)...

[" 2."CO_((g))+(1)/(2)O_(2)(g)rarr CO_(2(g))],[Delta H=-67.37K*cal" at "25^(@)C" the change in "],[" entropy accompanying process is -20.7caldeg "],[1mol^(-1)" then at "25^(@)C" the change in free energy "],[" 1) "-10K" .cal "mol^(-1)],[[" 3) "-32K" .cal "mol^(-1)," 2) - "-15K" .cal mole "^(-1)],[" ( the stan "]]

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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

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 :-

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)

C+O_(2)rarr CO_(2), Delta H = -94 K.cal, CO+(1)/(2)O_(2) rarr CO_(2), Delta H = -67.7 K.cal . On the basis of the above data, the heat of formation of 'CO' 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.

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.