List of top Chemistry Questions on Thermodynamics

An ideal gas expands from volume $V_{1}$ to $V_{2}$ through an isothermal reversible process. The work done by the system is given by

At constant temperature, one mole of an ideal gas of volume 2L expanded to 100 L against an external pressure of 1 atm under reversible conditions. What is the work done (in J)? (1 L atm = 101.3 J; \(\log 5 = 0.7\))

At T(K) in a reaction \(A(g) \rightarrow B(g) + C(g)\), x J of heat was absorbed and y J of work is done by the system. What is \(\Delta_r H\) (in J) for the reaction? (R= gas constant)

At 273 K the maximum work done when pressure on 10g of hydrogen is reduced from 10atm to 1 atm under isothermal, reversible conditions is

What is the work done (in J $mol^{-1}$) to vaporise 1 mole of $H_2O(l)$ to $H_2O(g)$ at 1 bar pressure and $100^{\circ}C$? ($\Delta_{vap}H = 41$ kJ $mol^{-1}$; $\Delta U = 37.9$ kJ $mol^{-1}$)

The signs of $\Delta$H and $\Delta$s for a reaction to be spontaneous at all temperatures respectively are

For which of the following process entropy change ($\Delta$S) is negative ?
• [I)] Sublimation of dry ice
• [II)] Freezing of water
• [III)] Crystallisation of the dissolved substance
• [IV)] Burning of rocket fuel

For a spontaneous process at constant temperature and pressure, the change in Gibbs free energy ($\Delta G$) is

At 273 K the maximum work done when pressure on 10g of hydrogen is reduced from 10atm to 1 atm under isothermal reversible conditions is

At constant temperature, one mole of an ideal gas of volume 2L was expanded to 100 L against an external pressure of 1 atm under reversible conditions. What is the change in internal energy? \((1 L atm=101.3~J; log~5=0.7)\)

For which of the following process entropy change ($\Delta S$) is negative ?
I) Sublimation of dry ice
II) Freezing of water
III) Crystallisation of the dissolved substance
IV) Burning of rocket fuel

Which of the following processes exhibits the decrease in internal energy of a system?

Calculate the change in internal energy if an ideal gas expands from \(0.5 \text{dm}^3\) to \(3.5 \text{dm}^3\) at constant pressure 2 bar by absorbing 1800 J heat energy.

A gas absorbs \(120\) J of heat and expands by \(300\times 10^{-6} \text{m}^3\) against a constant external pressure of \(2\times 10^5 \text{Nm}^{-2}\). What will be the change in internal energy of the system ?

Which of the following properties of a system depends upon the amount of matter and path?

In which of the following processes the internal energy of system remain constant?

Which of the following processes exhibits, \(\Delta U = 0\)?

Identify the correct statements from the following:

• Bomb calorimeter is used to determine the heat absorbed by water in a chemical reaction at constant volume

• Heat capacity is an extensive property

• The units of entropy are \(J\,K^{-1}\)
The correct answer is

Consider the following data for the reaction
$X_2(g) + Y_2(g) \rightleftharpoons 2XY(g)$
at 600 K. The $\Delta_r G^\ominus$ (in kJ $\text{mol}^{-1}$) for the reaction is :}

Match List-I with List-II.

Choose the correct answer.

List-I contains various physical/chemical processes, and List-II contains combinations of changes in enthalpy \((\Delta H)\) and entropy \((\Delta S)\). Match each entry in List-I to the appropriate entry in List-II and choose the correct option.

The signs of $\Delta H$ and $\Delta S$ for a reaction to be spontaneous at all temperatures respectively are

The number of extensive and intensive properties in the list given below is respectively:
Density, enthalpy, mass, temperature, volume, pressure

Calculate the work done in oxidation of 2 moles of \(SO_2\) at 298 K, if \(SO_{2(g) + \frac{1}{2}O_{2(g)} \rightarrow SO_{3(g)}\) [Given : R = 8.314 J/K/mol].}