For the reaction, ${{\rm{C}}_2}{{\rm{H}}_4}\left( {\rm{g}} \right) + 3{{\rm{O}}_2}\left( {\rm{g}} \right) \to 2{\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right) + 2{{\rm{H}}_2}{\rm{O}};$ ∆U=-1415 kJ. Then ∆H at ${27^0}$C is :

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

For the reaction,

{\mathrm{C}_2}{\mathrm{H}_4}\left( \mathrm{g} \right) + 3{\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + 2{\mathrm{H}_2}\mathrm{O};

∆U=-1415 kJ. Then ∆H at

{27^0}

C is :

View answer and explanation

Correct option: B

- 1420\mathrm{kJ}

Option B (- 1420 kJ) is correct because it correctly applies the relationship between ∆H and ∆U, accounting for the change in the number of moles of gas.

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