Calculate the heat of reaction at 298 K for the reaction $C_2{H}_{4(g)}+H_{2(g)}=C_2{H}_{6(g)}C\_2\; H\_\{4\; (g)\}\; +\; H\_\{2\; (g)\}\; =\; C\_2\; H\_\{6(g)\}$

Given that the heats of combustion of ethylene, hydrogen and ethane are 337.0, 68.4 and 373.0 kcal respectively.

Entropy change for a process is given by,

For a spontaneous process, total entropy change for a system and its surroundings is

For a system at equilibrium,

If the enthalpy of vaporisation of water at 100°C is 186.5 J·$mo{l}^{-1}mol^\{-1\}$ , the entropy of vaporization will be-

Heat of fusion of ice is 6.02kJmol-1 at 0 °C. If 100 g water is frozen at 0 °C, entropy change will be

If for a reaction $\mathrm{\Delta }H\backslash Delta\; H$ is negative and $\mathrm{\Delta }S\backslash Delta\; S$ is positive then the reaction is

Which of the following has highest entropy?

Gibbs free energy change at equilibrium is

For spontaneous process,