Thermodynamics practice · Mixed difficulty

Which of the following is a path function?

The magnitude of work done by one mole of a Van der Waals gas during its isothermal reversible expansion from volume $V_1$ to $V_2$ at temperature $T$ $\mathrm{K}$, is

Which of the following processes is an endothermic process?

Which of the following statements/expressions is/are correct?

∆H for the reaction given below represents, $\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{H}_2}\left( \mathrm{g} \right) \to \mathrm{CO}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right);\Delta \mathrm{H} = 40\mathrm{kJ}:$

The molar heat capacity of water at constant pressure is $75\mathrm{J}{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$ When 1.0 kJ of heat is supplied to 100 g of water which is free to expand the increase in temperature of water is

$\mathrm{C}_{\mathrm{p}} / \mathrm{C}_{\mathrm{v}}$ for noble gases is :

Among the following, the intensive properties are

(i) molar conductivity

(ii) electromotive force

(iii) resistance

(iv) heat capacity

Enthalpy of sublimation of iodine is $24\,\mathrm{cal}\,{g^{ - 1}}$ at ${200^\mathrm{o}}C$. If specific heat of ${I_2}\left( s \right)$ and ${I_2}\left( {\mathrm{vap}\mathrm{.}} \right)$ are 0.055 and 0.031 $\mathrm{cal }{g^{ - 1}}{K^{ - 1}}$ respectively, then enthalpy of sublimation of iodine at ${250^\mathrm{o}}C$ in $\mathrm{cal}\,{g^{ - 1}}$ is

${C_2}{H_6}\left( g \right) + \frac{7}{2}{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + 3{H_2}O\left( l \right);\,\Delta H = - 1560\,KJ$
${C_2}{H_2}\left( g \right) + \frac{5}{2}{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + {H_2}O\left( l \right);\,\Delta H = - 1310\,KJ$
${H_2}\left( g \right) + \frac{1}{2}{O_2}\left( g \right) \to {H_2}O\left( l \right);\Delta H = - 290\,KJ$
Enthalpy of hydrogenation of ethyne $\left( {{C_2}{H_2}} \right)$ is

When a $60 \, \mathrm{W}$ electric heater is immersed in a gas for $100 \, \text{s}$ in a constant volume container with adiabatic walls, the temperature of the gas rises by $5^{\circ} \mathrm{C}$. The heat capacity of the given gas is ______ $\mathrm{J} \, \mathrm{K}^{-1}$ (Nearest integer)

litre-atmosphere is equal to:

Statement - I: The final temperature of an ideal gas in adiabatic expansion is less in
reversible expansion than in irreversible expansion against a constant external pressure.

Statement - II: The magnitude of work done by an ideal gas in adiabatic expansion is more
in reversible process than that in irreversible process.

A: Work done in an irreversible isothermal process at constant volume is zero.
R: Work is assigned negative sign during expansion and is assigned positive sign during compression.

When 1 mole of gas is heated at constant volume. Temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct?

Given below are two statements one is labelled as Assertion (A) and the other is labelled as Reason (R)

Assertion (A): Heat of neutralisation of $HF$ (aq.) with ${NaOH}$ (aq.) is greater than $13.7 \mathrm{~Kcal}$.

Reason (R): Generally some heat is consumed in the ionisation of weak acid.
On the basis of above statements choose the most appropriate option from the following options:

Heat of combustion of $\mathrm{C}{\mathrm{H}_4},{\mathrm{C}_2}{\mathrm{H}_4},{\mathrm{C}_2}{\mathrm{H}_6}$ are - 890,-1411 and -1560 kJ/mol respectively. Which has the lowest calorific fuel value in kJ/g?

The temperature at which the reaction,
$\mathrm{A}{\mathrm{g}_2}\mathrm{O}\left( s \right) \to 2\mathrm{Ag}\left( s \right) + \frac{1}{2}{\mathrm{O}_2}\left( \mathrm{g} \right)$
Is at equilibrium is …;gives, $\Delta H = 30.5\,\,\;\mathrm{kJ\;mo}{\mathrm{l}^{ - 1}}$ and $\Delta S = 0.066\,\;\,\mathrm{kJ\;}\,{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$

The enthalpies of elements under the following conditions are assumed to be

Assertion : For a reaction

$2 {NH}_3({~g}) \longrightarrow {N}_2({~g})+3 {H}_2({~g}) ; \Delta H>\Delta E$

Reason : Enthalpy change is always greater than internal energy change.