NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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The correct thermochemical equation is :

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Correct option: C

\mathrm{C}\left( s \right) + {\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right);\Delta H = - 94\mathrm{kcal}

Option C (

\mathrm{C}( s ) + {\mathrm{O}_2}( \mathrm{g} ) \to \mathrm{C}{\mathrm{O}_2}( \mathrm{g} );\Delta H = - 94\mathrm{kcal}

) is correct because it represents the formation of carbon dioxide from its elements in their standard states (solid carbon and gaseous oxygen) with the correct negative sign for an exothermic reaction.

More Questions from THERMODYNAMICS

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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