NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

The enthalpy change for the following reaction. NaOH(aq)+HCl(aq)→NaCl(aq)+

{\mathrm{H}_2}\mathrm{O}

(l) is -57 kJ. Predict the value of the enthalpy change in the following reaction : Ba

{\left( {\mathrm{OH}} \right)_2}

{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}

(aq)→

\mathrm{BaS}{\mathrm{O}_4}

(s)+2

{\mathrm{H}_2}\mathrm{O}

(l)

View answer and explanation

Correct option: C

- 114\mathrm{kJ}

Option C (-114 kJ) is correct. The reaction involves the neutralization of a strong acid with a strong base, and since Ba(OH)₂ and H₂SO₄ are diprotic, the enthalpy change is twice that of the monoprotic reaction.

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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