A substance which shows highest entropy is

For a reaction, at 300K enthalpy is 138 kJ and entropy change is 115 $J{K}^{-1}JK^\{-1\}$ . Hence the free energy change of the reaction is

Bond enthalpies of $H_2{}^{-1}H\_2\{^\{-1\}\}$ , $I_{2(g)}I\_\{2(g)\}$ and HI are 436, 151 and 298 kJ $mo{l}^{-1}mol^\{-1\}$ respectively. Hence enthalpy of formation of $H{I}_{(g)}HI\_\{(g)\}$  is

The average bond energy of C-H bond is 410 $kJmo{l}^{-1}kJmol^\{-1\}$ . The enthalpy change of atomisation of $3.2g3.2\; \backslash \; g$  $C{H}_{4(g)}CH\_\{4(g)\}$ is

For a certain reaction, $\mathrm{\Delta }H\backslash Delta\; H$ = -50 kJ and $\mathrm{\Delta }S\backslash Delta\; S$ = -80 $J{K}^{-1}JK^\{-1\}$ , at what temperature does the reaction turn from spontaneous to non-spontaneous.

Third law of thermodynamics provides a method to evaluate which property?

One mole of which of the following has the highest entropy?

The species which by definition has ZERO standard molar enthalpy of formation at 298 K is

In a reversible process the system absorbs 600 kJ heat and performs 250 kJ work on the surroundings. What is the increase in the internal energy of the system?

In a system where $\mathrm{\Delta }E\backslash Delta\; E$ = -51.0 kJ, a piston expanded against a pext of 1.2 atm giving a change in volume of 32.0 L. What was the change in heat of this system?