Show that the reaction `CO(g) + 1/2 O_2(g) to CO_2(g)` at 300 K is spontaneous and exothermic, when the standard entropy change is `-0.094 kJ mol^-1 K^-1`. The standard Gibbs free energies of formation for `CO_2` and CO are -394.4 and `-137 kJ mol^-1`, respectively.

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

The standard entropy change for the reaction C_3H_(6(g)) + 9/2O_(2(g)) to 3CO_(2(g)) + 3H_2O_((l)) is – 339.23 JK-1 at 25^@C . Calculate the standard reaction enthalpy change if the standard Gibbs energy of formation of C_3H_(6(g)), CO_(2(g)) and H_2O_((l)) are 62.78, – 394.36 and –237.13 kJ. "mol"^(–1) respectively.

The standard entropy change Delta S_r^@ for CH_(4(g)) + 2O_(2(g)) to CO_(2(g)) + 2H_2O_((l)) is -242.98 JK^(-1) at 25^@C . Calculate the standard reaction enthalpy for the above reaction if standard Gibbs energy of formation of CH_(4(g)), CO_(2(g)) and H_2O_((l)) are -50.72, -394.36 and - 237.13 kJ mol^(-1) respectively.

Find out the heat of formation of CH_(3)CO OH . Given that the heat of Combustion of CH_(3)CO OH is -867 " kJ mol"^(-1) and the heat of formation of CO_(2) and H_(2)O are -393.5 and -285.9 " kJ mol"^(-1) respectively.

Find the value of DeltaG^(0) and K_(c) for the following reaction at 298K. NO(g)+(1)/(2)O_(2)(g)hArrNO_(2)(g) Given: standard free energy of formation (DeltaG_(f)^(0)) of NO_(2) and NO are 52.0 and 87.0 kJ*mol^(-1) respectively.

H_(2)O(l) to H_(2)(g)+(1)/(2)O_(2)(g) Does the above reaction occur spontaneously at 298 K ? Given that standard enthalpy of formation of water = -285.83 " kJ mol"^(-1) , standard entropy of H_(2)(g), O_(2)(g) and H_(2)O(l) are 130.57, 205.04 and 69.95 J. K^(-1). " mol"^(-1) respectively.

The following reaction is performed at 298 K. 2NO(g) + O_2(g) rarr 2NO_2(g) The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO_2(g) at 298 K?( K_p = 1.6 xx 10^(12) )

At 25^(@)C , the standard heat of formation for Br_(2)(g) is 30.9kJ*mol^(-1) . At this temperature, the heat of vaporisation for Br_(2)(l) is-