NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

1 of 1

Application +4 | -1

Calculate the work done by

16g

of oxygen gas (assuming ideal behaviour) of molar mass

32\,\,g.mo{l^{ - 1}}

undergoing isothermal reversible expansion at

300K

from an initial volume

2.5L

to final volume

2.5L

( in the L. atm)

\left( {R = 8.2 \times {{10}^{ - 2}}\,\,L\,\,atm} \right)

View answer and explanation

Correct option: A

- 2872\,\,J

Option A (-2872 J) is correct because it is the result of calculating the work done during an isothermal reversible expansion using the ideal gas law.

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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