Thermodynamics practice · Mixed difficulty

In a closed container, a liquid is stirred with a paddle to increase the temperature. Which of the following is true?

The enthalpy of formation steadily changes from $-17.89 \mathrm{~Kcal} / \mathrm{mol}$ to $-49.82 \mathrm{~Kcal} / \mathrm{mol}$ as we go from $\mathrm{CH}_4, \mathrm{C}_2 \mathrm{H}_6$ to $\mathrm{C}_8 \mathrm{H}_{18}.$ The value of $\Delta G$ however shows opposite trend from $-12.12 \mathrm{~Kcal} /\mathrm{mol}$ for $\mathrm{CH}_4$ to $4.14 \mathrm{~Kcal} / \mathrm{mol}$ for $\mathrm{C}_8 \mathrm{H}_{18}.$ Why?

When one mole of monoatomic ideal gas at T temperature undergoes adiabatic change under a constant external pressure of 1 atm change in volume is from 1 L to 2 L, the final temperature in Kelvin would be

The internal energy change when a system goes from state A to B is 40 kJ/mol. If the system goes from A to B by a reversible path and returns to state A by an irreversible path, what would be the net change in internal energy?

For the reversible process, the value of $\Delta S$ is given by the expression

Work done by the system on surroundings is:

In previous problem if expansion is carried out freely $\left(P_{\mathrm{ext}}=0\right)$, then $\Delta S$ is :

The correct thermochemical equation is :

The enthalpies of neutralization of a weak base $\mathrm{AOH}$ and a strong base $\mathrm{BOH}$ by $\mathrm{HCl}$ are $-12250 \mathrm{cal} / \mathrm{mol}$ and $-13000 \mathrm{cal} / \mathrm{mol}$ respectively. When one mole of $\mathrm{HCl}$ is added to a solution containing 1 mole of $A O H$ and 1 mole of $B O H$, the enthalpy change was $-12500 \mathrm{cal} / \mathrm{mol}$. In what ratio is the acid distribution between $A O H$ and $B O H$ ?

If a gas has 2 atm and 5 atm pressure at 30℃ and 27℃ respectively. Then it will

Two atoms of hydrogen combine to form a molecule of hydrogen gas, the energy of the ${H_2}$ molecule is :

When water is added to quick lime, the reaction is :

What is the enthalpy change for, $2 {H}_2 {O}_2(l) \rightarrow 2 {H}_2 {O}(l)+{O}_2(g)$ if heat of formation of ${H}_2 {O}_2(l)$ and ${H}_2 {O}(l)$ are -188 and $-286 {~kJ} / {mol}$ respectively?

$S + \frac{3}{2}{O_2} \to S{O_3} + 2x\,\,kcal.....\left( i \right)\,\,\,\,S{O_2} + \frac{1}{2}{O_2} \to S{O_3} + y\,\,kcal.....\left( {ii} \right)$
Find out the Enthalpy of formation of $S{O_2}$:

A system absorbs 10 kJ of heat and does 4 kJ of work. The internal energy of the system

The value of $\Delta H$ for the reversible isothermal evaporation of $90 \mathrm{~g}$ water at $100^{\circ} \mathrm{C}$ will be

For the reaction,
$\begin{array}{l} {\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to 2\mathrm{HCl}\left( \mathrm{g} \right) + {x_1}\,\,\mathrm{kJ} \ldots \ldots \ldots \left( \mathrm{i} \right)\\ 2\mathrm{HCl}\left( \mathrm{g} \right) \to {\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) - {x_2}\,\mathrm{kJ} \ldots \ldots \left( {\mathrm{ii}} \right) \end{array}$
Which of the following statement is correct?

Net work done by the system in a cyclic process is equal to:

Consider the following statements for the reaction between zinc and oxygen.

$\begin{aligned} & 2 \mathrm{Zn(s})+\mathrm{O}_2(\mathrm{g}) \longrightarrow 2 \mathrm{ZnO(s}) ; \\ & \Delta H=-693.8 \mathrm{~kJ~mol}^{-1} \end{aligned}$

I. The enthalpy of two moles of $\mathrm{ZnO}$ is less than the total enthalpy of two moles of $\mathrm{Zn}$ and one mole of oxygen by $693.8 \mathrm{~kJ}$

II. The enthalpy of two moles of $\mathrm{ZnO}$ is more than the total enthalpy of two moles of $\mathrm{Zn}$ and one mole of oxygen by $693.8 \mathrm{~kJ}$

III. $693.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$ energy is evolved in the reaction

IV. $693.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$ energy is absorbed in the reaction

Select the correct statements and choose the correct option.

The molar heat capacity of a diatomic gas at constant pressure is :

The Kirchhoff’s equation gives the effect of …..on heat of reaction.

The bond energy of ${H_2}$ is 104.3 kcal $mo{l^{ - 1}}.$. It means : (N=Av.no.)

Which is correct relation between $\mathrm{C}_{\mathrm{p}}$ and $\mathrm{C}_{\mathrm{v}}$ for one mole of ideal gas

Which among the following equations
represents the first law of thermodynamics
under isobaric conditions?

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298K To 308K. The change in internal energy is:

Which is not correct?

A system is provided 50 J of heat and work done on the system is 10 J. what is the change in internal energy

The molar heat capacity at $25^{\circ} \mathrm{C}$ should be close to $27 \mathrm{~J} / \mathrm{K}-\mathrm{mol}$ for all of the given elements except

To what pressure a certain volume of $\mathrm{Cl}_2$ originally at $373 \mathrm{~K}$ and 1 bar pressure be adiabatically compressed in order to raise its temperature to $673 \mathrm{k} . C_P / C_r$ for $\mathrm{Cl}_2$ is 1.4

The heat of combustion of rhombic and monoclinic sulphur are 70.96 and 71.03 kcal. The heat of transition of ${S_{R \to M}}$ is: