Thermodynamics practice · Mixed difficulty

2 mole of an ideal gas undergo isothermal and reversible expansion from 2 litre to 20 liltre at $127^{\circ} \mathrm{C}$ the work done by the gas is

In thermodynamics, a quantity whose value
simply depends upon the initial and final states
of the system is called

Heat energy change during the chemical reaction, $\mathrm{CO} + \frac{1}{2}{\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2}$is known as :

A thermally isolated gaseous system can exchange energy with the surroundings. The mode of transference of energy can be:

For the reaction, ${\mathrm{N}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\left( \mathrm{g} \right) \to 2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right),$ which is true?

Work done in reversible adiabatic process is given by:

The van’t Hoff reaction isotherm is:

Given are two statements one is labelled as Assertion A and other is labelled as Reason R.
Assertion A: Magnesium can reduce $A{l_2}{O_3}$ at a temperature below $1350^\circ \,C$, while above $1350^\circ \,C$ aluminium can reduce $MgO$.
Reason R: The melting and boiling points of magnesium are lower than those of aluminium.
In light of the above statements, choose most appropriate answer from the options given below:

Given, $\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2} + 94.2\mathrm{kcal} \ldots \mathrm{.}\left( \mathrm{i} \right)$${\mathrm{H}_2} + \frac{1}{2}{\mathrm{O}_2} \to {\mathrm{H}_2}\mathrm{O} + 68.3\mathrm{kcal} \ldots .\left( {\mathrm{ii}} \right)$$\mathrm{C}{\mathrm{H}_4} + 2{\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2} + 2{\mathrm{H}_2}\mathrm{O} + 210.8\mathrm{kcal} \ldots \mathrm{.}\left( {\mathrm{iii}} \right)$The heat of formation in kcal will be :

The heat change for a reaction $CO\left( g \right) + \frac{1}{2}{O_2}\left( g \right)\,\xrightarrow{\,}\,C{O_2}\left( g \right)$ refers to

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0℃ is:

For the melting of $NaCl$ heat required is $7.26\,K\,cal\,mo{l^{ - 1}}$ and $\Delta S$ increases by $6.73\,cal\,mo{l^{ - 1}}.{K^{ - 1}}.$ The melting point of the salt is

If we take water at temperature $T_A$ in a container having thermally conducting walls and enclosed in a huge heat reservoir at temperature $T_B$. What is the correct expression of change in internal energy if no work is done at constant volume?

Statement - I: In an adiabatic expansion of an ideal gas, the entropy of the surrounding
remains unchanged independent whether the expansion is reversible or irreversible.

Statement - II: In an adiabatic process, the surrounding does not exchange heat with the
system and the process may be reversible or irreversible for system but it always remain
reversible for the sorrounding.

Which of the following is an example of extensive property?

The heat change taking place during the reaction $\;{\mathrm{H}_2}\mathrm{O}\left( l \right)$$\to {\mathrm{H}_2}\mathrm{O(g)}$ is: [Given,$\Delta {H_f}$ of ${\mathrm{H}_2}\mathrm{O}(g)$ = -57 kcal, $\Delta {H_f} = {\mathrm{H}_2}\mathrm{O}\left( l \right)$ = -68.3 kcal]

For the reaction; $\;{\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}\left( l \right) + 3{\mathrm{O}_2}\left( \mathrm{g} \right) \to \;2C{O_2}(g) + 3{H_2}O(l)$ which one is true?

A gas is allowed to expand under reversible adiabatic conditions then :-

What is the entropy change in $\mathrm{JK}^{-1}$ during the melting of $27.3 \mathrm{~g}$ of ice at $0^{\circ} \mathrm{C}$ ? (Latent heat of fusion of ice $=330 \mathrm{Jg}^{-1}$ )

How much heat (in kJ) is evolved when 2.7 g of aluminium reacts with a stoichiometric amount of $\mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3}$?$2\mathrm{A}{\mathrm{l}_2} + \mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3} \to 2\mathrm{Fe} + \mathrm{A}{\mathrm{l}_2}{\mathrm{O}_3};\Delta {H^o} = - 852\,\mathrm{kJ}$

A solution of 500 mL of 2M KOH is added to 500 mL of 2M HCl and the mixture is well shaken. The rise in temperature $\;{T_1}$ is noted. The experiment is then repeated using 250 mL of each solution and rise in temperature $\;{T_2}$ is again noted. Assume all heat is taken up by the solution:

Heat of combustion ∆H for C(s), ${\mathrm{H}_2}$(g) and $\mathrm{C}{\mathrm{H}_4}$ (g) are -94,-68 and -213 kcal/mole then ∆H for $\mathrm{C}\left( s \right) + 2{\mathrm{H}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{H}_4}\left( \mathrm{g} \right)\mathrm{i}s:$

Molar heat capacity is given by :

Consider the following equation, $q=\text { coeff. } \times \Delta T$. The magnitude of the coefficient depends on

The heat of formation is the change in enthalpy accompanying the formation of a substance from its elements at 298 K and 1 atm pressure. Since, the enthalpies of elements in their most stable state are taken to be zero, the heat of formation of compounds is :

To calculate the amount of work done in joules during reversible isothermal expansion of an ideal gas, the volume must be expressed in

Hess’s law is related to:

Identify the correct statement for change of Gibb’s energy for a system ($\Delta {G_{\mathrm{system}}}$) at constant temperature and pressure:

$56 \mathrm{~g}$ of iron reacts with $\mathrm{HCl}$ in a closed vessel of fixed volume. Again, same amount of $\mathrm{Fe}$ is made to react in an open beaker at $27^{\circ} \mathrm{C}$. The work done (in cal) in both the cases will be respectively

Heat of neutralization of a strong acid $H A$ and a weaker acid $H B$ with $K O H$ are -13.7 and $-12.7 \mathrm{K} \mathrm{cal} \mathrm{mol}^{-1}$. When 1 mole of $\mathrm{KOH}$ is added to a mixture containing 1 mole each of $H A$ and $H B$, the heat changes was $-13.5 \mathrm{K}$ cal. In what ratio is the base distributed between $H A$ and $H B$.