Thermodynamics practice · Mixed difficulty

During isothermal expansion of one mole of an ideal gas from $10 {~atm}$ to $1 {~atm}$ at $273 {~K}$, thework done is (gas constant $=2$ ) :

A gas expands against a variable pressure given by $P=\frac{20}{V}$ (where $P$ in atm and $V$ in $\mathrm{L}$ ). During expansion from volume of 1 litre to 10 litre, the gas undergoes a change in internal energy of $400 \mathrm{~J}$. How much heat is absorbed by the gas during expansion?

The heat of neutralisation for strong acid and strong base forming 2 moles of water is

The law of Lavoisier and Laplace is based on :

At $298 \mathrm{~K}$ what will be the change in standard internal energy change for the given reaction $\mathrm{OF}_2(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{O}_2(\mathrm{~g})+2 \mathrm{HF}(\mathrm{g}) ;$

The gas in a refrigerator causes cooling on expansion because:

Energy equivalent to one erg, one joule and one calorie are in order:

Work done in reversible adiabatic process is given by:

For an isothermal reversible expansion process, the value of $q$ can be calculated by the expression

The heat of combustion of ethanol into carbon dioxides and water is $- 327\,\,kcal$ at constant pressure. The heat evolved (in cal) at constant volume and ${27^\mathrm{o}}\,\,C$ (if all gases behave ideally) is ($R = 2$ cal $mo{l^{ - 1}}\,{K^{ - 1}}$ )……

At $27^{\circ} \mathrm{C}$ the reaction, ${C}_6 {H}_{6}({l})+15 / 2 {O}_{2}({g}) \rightarrow 6 {CO}_{2}({g})+3 {H}_2 {O}{({l})}$ proceeds spontaneously because the magnitude of

In an isobaric process, when temperature change from $\mathrm{T}_1$ to $\mathrm{T}_2, \Delta \mathrm{S}$ is equal to:

An ideal monoatomic gas initially at $300 \mathrm{~K}$ expands adiabatically into vacuum to double its volume. The final temperature of gas is

Choose the reaction in which $\Delta {H}$ is not equal to $\Delta {U}$ ?

Which of the following represents the first law
of thermodynamics

For the reaction $2Cl\left( g \right) \to C{l_2}\left( g \right),$ the signs of $\Delta H$ and $\Delta S$ respectively are

Calculate the standard internal energy change for the following reaction at $25^{\circ} \mathrm{C}$.

$\begin{aligned} & 2 \mathrm{H}_2 \mathrm{O}_2(\mathrm{l}) \longrightarrow 2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{O}_2(\mathrm{g}) \\ & \mathrm{H}_2 \mathrm{O}_2(\mathrm{l})=-188.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \mathrm{H}_2 \mathrm{O}(\mathrm{l})=-286.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \left(\mathrm{R}=8.314 \mathrm{~J~K}^{-1} \mathrm{~mol}^{-1}\right) \end{aligned}$

$1 \mathrm{~g~H}_2$ gas at S.T.P. is expanded so that volume is doubled. Find the work done in Joules. (1 litre atm = $101.3 \mathrm{~J}$)

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

Considering entropy(s) as the thermodynamic parameter, the criterion for the spontaneity of any process is:

For the dissociation reaction, $\mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g}), \Delta \mathrm{H}=162 \mathrm{Kcal}$, heat of atomization of $\mathrm{H}$ is

The standard molar enthalpies of formations of $\mathrm{H}_2 \mathrm{O}({l})$ and $\mathrm{H}_2 \mathrm{O}_2({l})$ are $-286$ and $-188 \mathrm{~kJ} / \mathrm{mol},$ respectively. Molar enthalpies of vaporization of $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{H}_2 \mathrm{O}_2$ are $44$ and $53 \mathrm{~kJ},$ respectively. The bond dissociation enthalpy of $\mathrm{O}_2(\mathrm{g})$ is $498 \mathrm{~kJ} / \mathrm{mol}.$ Calculate the bond dissociation enthalpy of $\mathrm{O}-\mathrm{O}$ bond in $\mathrm{H}_2 \mathrm{O}_2,$ assuming that the bond dissociation enthalpy of $\mathrm{O}-\mathrm{H}$ bond is same in both $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{H}_2 \mathrm{O}_2.$

Determine $\Delta G^{\circ}$ for the following reaction

$\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$

$\Delta H^{\circ}=-282.84 \mathrm{~kJ} \text { given, } \mathrm{S}^{\circ} \mathrm{CO}_2=213.8$

$\mathrm{~S}^{\circ} \mathrm{O}_2=205.8 \mathrm{JK} / \mathrm{mol}$

A gas, while expanding absorbs $25 \mathrm{~J}$ of heat and does $243 \mathrm{~J}$ of work. Thus, $\Delta E$ (change in internal energy) for the gas is

For a perfectly crystalline solid $C_{p, m}=a T^3$, where $a$ is constant. If $C_{p, m}$ is $0.42 \mathrm{~J} / \mathrm{K} \mathrm{~mol} \mathrm{~at} 10 \mathrm{~K}$, molar entropy at $20 \mathrm{~K}$ is :

Consider the following conversions:

(i) $\mathrm{O}_{(g)}+e^{-} \rightarrow O^{-}(g), \Delta H_1$

(ii) $\mathrm{F}_{(g)}+e^{-} \rightarrow F^{-}(g), \Delta H_2$

(iii) $\mathrm{Cl}_{(\mathrm{g})}+\mathrm{e}^{-} \rightarrow \mathrm{Cl}^{-}(\mathrm{g}), \Delta \mathrm{H}_3$

(iv) $\mathrm{O}_{(g)}^{-}+e^{-} \rightarrow O^{2-}(g), \Delta H_4$

That according to given information the incorrect statements is:

A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If ∆H is the enthalpy change and ∆E is the change in internal energy, then

Standard entropy of $X_2, Y_2$ and $X Y_4$ are 30, 60 and $110 \mathrm{~J} / \mathrm{K} \mathrm{~mol}$ respectively. For the reaction $\frac{1}{2} \mathrm{X}_2+2 \mathrm{Y}_2 \rightarrow \mathrm{XY}_4, \Delta \mathrm{H}=-40 \mathrm{~kJ}$. To be at equilibrium, the temperature will be:

An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If ${T_i}$ is the initial temperature and ${T_f}$ is the final temperature, which of the following statements is correct?

Which is an extensive property of the system?