The value of ∆E for combustion of 16 g of ${\rm{C}}{{\rm{H}}_4}$ is -885389 J at 298 K. The ∆H combustion for ${\rm{C}}{{\rm{H}}_4}$ in J ${\rm{mo}}{{\rm{l}}^{ - 1}}$ at this temperature will be (Given that, R=8.314 ${\rm{J}}{{\rm{K}}^{ - 1}}$ ${\rm{mo}}{{\rm{l}}^{ - 1}}$)

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

1 of 1

Application +4 | -1

The value of ∆E for combustion of 16 g of

\mathrm{C}{\mathrm{H}_4}

is -885389 J at 298 K. The ∆H combustion for

\mathrm{C}{\mathrm{H}_4}

in J

\mathrm{mo}{\mathrm{l}^{ - 1}}

at this temperature will be
(Given that, R=8.314

\mathrm{J}{\mathrm{K}^{ - 1}}

\mathrm{mo}{\mathrm{l}^{ - 1}}

)

View answer and explanation

Correct option: B

- 880430

Option B (-880430 J

\mathrm{mo}{\mathrm{l}^{ - 1}}

) is correct because it calculates the enthalpy change for the combustion of one mole of methane using the given energy change and accounting for the difference between

\Delta E

and

\Delta H

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

More Questions from THERMODYNAMICS