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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1
If ΔHf∘\Delta H_f^\circ for H2O2{H}_2 {O}_2 and H2O{H}_2 {O} are −188KJ/mol-188 {KJ} / \mathrm{mol} and −286KJ/mol-286 {KJ} / \mathrm{mol}, what will be the enthalpy change of the reaction

2H2O2(l)→2H2O(l)+O2(g)2 {H}_2 {O}_2({l}) \rightarrow 2 {H}_2 {O}({l})+{O}_2(g)
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Correct option: A
−196 KJ-196 \,{KJ}
Option A (-196 KJ) is the correct answer because it is calculated using the enthalpy of formation values for the products and reactants.

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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 Ti{T_i} is the initial temperature and Tf{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 H2O(s)→H2O(g)\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, X2O4(l)⟶2XO2(g),ΔU=2.1 kcal,ΔS=20 cal K−1\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} at 300 K300 \mathrm{~K}. Hence, ΔG\Delta G is
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