Thermodynamics practice · Mixed difficulty

Assertion :- Sum of two path functions is always path function.

Reason :- Sum of path function depends on path followed.

The heat change for the reaction,${\mathrm{H}_2}\mathrm{O}\left( l \right)$$\to \;{\mathrm{H}_2}\mathrm{O}\;(g)$ is called as :

Mark out the enthalphy of formation of carbon monoxide (CO)Given,$\mathrm{C}\left( s \right) + {\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{CO}\left( \mathrm{g} \right)\;,\Delta H = - 393.3\;kJ/mol$
$\mathrm{CO}\left( \mathrm{g} \right) + \frac{1}{2}{\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right),\Delta H = - 282.8\mathrm{kJ}/\mathrm{mol}$

The entropy of the universe:

The difference between heat of reaction at constant pressure and constant volume for the reaction given below at $25^\circ C$ in kJ is:
$2{C_6}{H_6}(l) + 15{O_2}(g)\xrightarrow{\,}\,12C{O_2}(g) + 6{H_2}O(l)\,$

The quantity of heat (in $J$ ) required to raise the temperature of $1.0 \mathrm{~kg}$ of ethanol from $293.45 \mathrm{~K}$ to the boiling point and then change to liquid to vapour at that temperature is closest to [Given, boiling point of ethanol $351.45 \mathrm{~K}$. Specific heat capacity of liquid ethanol $2.44 \mathrm{~J} \mathrm{~g}^{-1} \mathrm{k}^{-1}$. Latent heat of vaporisation of ethanol $855 \mathrm{~J} \mathrm{~g}^{-1}$ ]

If '$x$' mole of ideal gas at $27^\circ C$ expands isothermally and reversibly from a volume of '$y$' to $10 y$, then work done is

Which of the following is a highly corrosive salt?

One mole of $\mathrm{CH}_3 \mathrm{COOH}$ undergoes dimerization in vapour phase at $127^{\circ} \mathrm{C}$ as:

$2 \mathrm{CH}_3 \mathrm{COOH}(\mathrm{g}) \rightleftharpoons\left(\mathrm{CH}_3 \mathrm{COOH}\right)_2(\mathrm{~g})$

if dimer formation is due to two $\mathrm{H}$-bonds involved in dimer, each of $33 \mathrm{~kJ}$ stength and the degree of dimerisation of acetic acid $98.2 \%$. The change in standard entropy during dimerization is

Enthalpies of formation of $\mathrm{CCl}_{4}(\mathrm{g}), \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$, $\mathrm{CO}_{2}(\mathrm{g})$ and $\mathrm{HCl}(\mathrm{g})$ are $-105,-242,-349$ and -92 $\mathrm{kJ} \mathrm{mol}^{-1}$ respectively. The magnitude of enthalpy of the reaction given below is _____ $\mathrm{kJ}$ $\mathrm{mol}^{-1}$. (Nearest integer)
$\mathrm{CCl}_{4}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+4 \mathrm{HCl}(\mathrm{g})$

Which of the following is an intensive property?

Two bars of different metals are heated to $60^{\circ} \mathrm{C}$ and then immersed in identical insulated containers each containing $200 \mathrm{~g}$ of water at $20^{\circ} \mathrm{C}.$ Will the metal with higher or lower atomic mass cause a greater temperature rise in water?

In a irreversible process, the value of $\Delta {S_{\mathrm{System}}} + \Delta {S_{\mathrm{Surroundings}}}$ is

Hess’s law is used to calculate

Work done by an ideal gas at a constant
volume is .........

Select the path function among the following.

Assertion : Molar enthalpy of vaporisation of water is different from ethanol.

Reason : Water is more polar than ethanol.

For adiabatic expansion of a perfect gas $\frac{d P}{P}$ is :

An exothermic reaction is one in which the reacting substances

Heat of reaction at constant volume is equal to :

A gas is allowed to expand in an insulated container against a constant external pressure of 4 atm from the initial volume of 1.8 L to a final volume of 5.2 L. The change in internal energy of the gas is

The heat of formation of water is exothermic in nature because :

From the reaction, ${\mathrm{P}_{\left( {\mathrm{white}} \right)}} \to {\mathrm{P}_{\left( {\mathrm{red}} \right)}};$ ∆H= -18.4 kJ it following that :

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 $4.2\,kJ\,{K^{ - 1}}\,k{g^{ - 1}}$ and $20\,kJ\,{K^{ - 1}}\,k{g^{ - 1}}$; heat of liquid fusion and vapourisation of water are $334\,kJ\,k{g^{ - 1}}\mathrm{ }$ and $2491\,kJ\,k{g^{ - 1}}$ respectively).
$(\log 273 = 2.436,\,\,\log 373 = 2.572,\,\,\log 383 = 2.583)$

When an electric current of $0.50 \mathrm{~A}$ from a $12 \mathrm{~V}$ supply is passed for $\frac{1805}{6} \mathrm{sec}$ through a resistance in thermal contact with water maintained at 1 atm and $373 \mathrm{~K},$ it is found that $0.9 \mathrm{~g}$ of water is vaporized. The molar internal energy change of water is (Take $8.314 \times 373=3100$)

50 mL of water takes 5 min to evaporate from a vessel on a heater connected to an electric source which delivers 400 W. The enthalpy of vaporisation of water is

The Gibbs energy change for a reversible reaction at equilibrium is:

The bond energies of ${\mathrm{F}_2}$,$\mathrm{C}{\mathrm{l}_2},\mathrm{B}{\mathrm{r}_2}$ and ${\mathrm{I}_2}$ are 155.4, 243.6, 193.2 and 151.2 kJ $\mathrm{mo}{\mathrm{l}^{ - 1}}$ respectively. The strongest bond is :

Assertion: In a process, if work $=0$ then $\Delta U=$ q.

Reason: $q$ is difference between initial state and final state of a system.

For a spontaneous process, entropy :