Thermodynamics

Lattice enthalpy and enthalpy of solution of NaCl are 788 kJ mol^–1, and 4 kJ mol^–1, respectively. The hydration enthalpy of NaCl is :

The process that is NOT endothermic in nature is :

If enthalpy of atomisation for Br_2(1) is x kJ/mol and bond enthalpy for Br₂ is y kJ/mol, the relation between them :

At 25$^\circ$C and 1 atm pressure, the enthalpy of combustion of benzene (I) and acetylene (g) are $-$ 3268 kJ mol^$-$1 and $-$1300 kJ mol^$-$1, respectively. The change in enthalpy for the reaction 3 C₂H₂(g) $\to$ C₆H₆ (I), is :

At 25$^\circ$C and 1 atm pressure, the enthalpies of combustion are as given below : .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} Substance ${H_2}$ C (graphite) ${C_2}{H_6}(g)$ ${{{\Delta _c}{H^\Theta }} \over {kJ\,mo{l^{ - 1}}}}$ $- 286.0$ $- 394.0$ $- 1560.0$ The enthalpy of formation of ethane is

Given .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-0lax{text-align:left;vertical-align:top} (A) $\mathrm{2CO(g)+O_2(g)\to 2CO_2(g)}$ $\mathrm{\Delta H_1^0=-x~kJ~mol^{-1}}$ (B) $\mathrm{C(graphite)+O_2(g)\to CO_2(g)}$ $\mathrm{\Delta H_2^0=-y~kJ~mol^{-1}}$ $\mathrm{\Delta H^0}$ for the reaction $\mathrm{C(graphite)+\frac{1}{2}O_2(g)\to CO(g)}$ is :

Given below are two statements: One is labelled as Assertion (A) and the other is labelled as Reason (R) Assertion (A) : Enthalpy of neutralisation of strong monobasic acid with strong monoacidic base is always $-57 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Reason (R) : Enthalpy of neutralisation is the amount of heat liberated when one mole of $\mathrm{H}^{+}$ ions furnished by acid combine with one mole of ${ }^{-} \mathrm{OH}$ ions furnished by base to form one mole of water. In the light of the above statements, choose the correct answer from the options given below.

The entropy change associated with the conversion of 1 kg of ice at 273 K to water vapours at 383 K is : (Specific heat of water liquid and water vapour are 4.2 kJ K^$-$1 kg^$-$1 and 2.0 kJ K^$-$1 kg^$-$1; heat of liquid fusion and vapourisation of water are 334 kJ^$-$1 and 2491 kJ kg^$-$1, respectively). (log 273 = 2.436, log 373 = 2.572, log 383 = 2.583)

The process with negative entropy change is :

Two blocks of the same metal having same mass and at temperature T₁ and T₂, respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta$S, for this process is :