At 25$°$C, for the process H₂O(l)$\rightleftharpoons$H₂O(g);

$∆\mathrm{G}°$ is 8.6 kJ. The vapour pressure of water at this temperature is nearly:-

1. 24 torr

2. 285 torr

3. 32.17 torr

4. 100 torr

What will be the standard enthalpy of reaction for the following reaction using the listed enthalpies of reaction?

3Co(s) + 2O₂(g)$\to$Co₃O₄(s);       $∆\mathrm{H}$=?

2Co(s) + O₂(g) $\to$2CoO(s)          $∆{\mathrm{H}}_1$= -475.8 KJ

6CoO(s) + O₂(g) $\to$2Co₃O₄(s)    $∆{\mathrm{H}}_2$ = -355.0 KJ

1. -891.2 KJ

2. -120.8 KJ

3. 891.2 KJ

4. -830.8 KJ

For given following equations and $∆\mathrm{H}°$ values, determine the enthalpy of reaction at 298 K for the reaction 

C₂H₄(g) + 6F₂(g) $\to$ 2CF₄(g) + 4HF(g)

H₂(g) + F₂(g) $\to$ 2HF(g)       $∆{\mathrm{H}}_1^{°}$= -537 kJ

C(s) + 2F₂(g) $\to$CF₄(g)         $∆{\mathrm{H}}_2^{°}$=-680 kJ

2C(s) + 2H₂(g) $\to$C₂H₄(g)    $∆{\mathrm{H}}_3^{°}$= 52 kJ

1. -1165 

2. -2486

3. +1165

4. +2486

If $∆{\mathrm{H}}_{\mathrm{f}}^{°}$(C₂H₄) and $∆{\mathrm{H}}_{\mathrm{f}}^{°}$(C₂H₆) are x₁ and x₂ kcal/mol then heat of hydrogenation of C₂H₄ is :-

(1) x₁ + x₂

(2) x₁ - x₂

(3) x₂ - x₁

(4) x₁ + 2x₂

The following reaction is given for reference:
4Fe(s) + 3O₂(g)  → 2Fe₂O₃(s)
Also, for the oxidation of iron at 298 K, $∆{\mathrm{H}}_{\mathrm{r}}^{°}$=-1648 x 10³ J mol^-1 & ∆S= -549.4 J K^-1mol^-1.

Based on the data given above, it can be concluded that the nature of the reaction is:

1. Spontaneous
2. Non-spontaneous
3. At Equilibrium
4. The nature of the reaction cannot be predicted.

18 g of ice is converted into water at 0$°$C and 1 atm. The entropy of H₂O_(s) and H₂O_(l) are 38.2 and 60 J K^-1 mol^-1 respectively. the enthalpy for this conversion will be

(1) 5951.4 J/mol

(2) 595.14 J/mol

(3) -595.14 J/mol

(4) None of these

One mole of methanol when burnt in O₂ gives out 723 kJ mol^-1 of heat. If one mole of O₂ is used, what will be the amount of heat evolved?

1. 482 kJ
2. 241 kJ
3. 723 kJ               
4. 924 kJ

If the bond energies of H-H, Br-Br, and H-Br are 433, 192 and 364 kJ mol^-1 respectively, 

the $∆\mathrm{H}°$ for the reaction

H₂(g) + Br₂(g) $\to$2HBr(g) is

1.  -103 kJ               

2. -261 kJ

3. +103 kJ               

4. +261 kJ

For isothermal expanison in case of an ideal gas:-

(1) $∆$G=$∆$S

(2) $∆$G=$∆$H

(3) $∆$G=-T$∆$S

(4) None of these

The free energy change $∆\mathrm{G}$=0 when:-

(1) The system is at equilibrium

(2) Catalyst is added

(3) Reactants are initially mixed throughly

(4) The reactants are completely consumed