The enthalpy of formation of methane at constant pressure and $300 K$ is $- 75.83 k J$ . What will be the heat of formation at constant volume?
$(R = 8.3 J {m o l}^{- 1} K^{- 1})$

53.34 k J

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- 53.34 k J

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73.34 k J

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- 73.34 k J

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Solution

The correct option is D $- 73.34 k J$
We have,
$Δ H = Δ U - R T$
-75830 = $Δ U - 8.314 * 300$
$h e a t o f f o r m a t i o n a t c o n s t a n t v o l u m e = - 73340 J o r - 73.34 K J$

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The enthalpy of formation of methane at constant pressure and $300 K$ is $- 75.83 K J$ . What will be the heat of formation at constant volume? $(R = 8.3 J K^{- 1} m o l^{- 1}$ )

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The enthalpy of formation of methane at constant pressure and 300K is −75.83kJ. What will be the heat of formation at constant volume?(R=8.3Jmol−1K−1)

The correct option is D −73.34kJWe have,ΔH=ΔU−RT-75830 = ΔU−8.314∗300heatofformationatconstantvolume=−73340Jor−73.34KJ

The enthalpy of formation of methane at constant pressure and $300 K$ is $- 75.83 k J$ . What will be the heat of formation at constant volume?
$(R = 8.3 J {m o l}^{- 1} K^{- 1})$

The correct option is D $- 73.34 k J$
We have,
$Δ H = Δ U - R T$
-75830 = $Δ U - 8.314 * 300$
$h e a t o f f o r m a t i o n a t c o n s t a n t v o l u m e = - 73340 J o r - 73.34 K J$