NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Medium

1 of 1

Application +4 | -1

For a reversible process at T=300 K, the volume of 2 mole of ideal gas is increased from 1 litre to 10 litre, the ∆H for isothermal change is:

View answer and explanation

Correct option: B

4.98 kJ

Option C (0) is correct because for an isothermal process with an ideal gas, the enthalpy change (∆H) is zero since enthalpy depends only on temperature.

More Questions from THERMODYNAMICS

Practice All Chapter MCQs →

The internal energy of one mole of a gas is: 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? For which of the process, ∆S is negative? The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by: Assertion :- At constant pressure of the change

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

work done is negative.

Reason :- During phase transition work done is always negative. For the reaction,

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

. Hence,

\Delta G