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Standard XII

Chemistry

Difference between Internal Energy and Enthalpy

One mole of a...

Question

One mole of a non-ideal gas undergoes change of state (2.0 atm, 3.0 L, 95 K) $\to$ (4.0 atm, 5.0L, 245 K) with a change in enthalpy 44 L $-$ atm. Calculate the change in internal energy $(Δ U)$ in L $-$ atm. Give the answer as $x$ , where $x = Δ U \times \frac{1}{10} .$

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Solution

$Δ U = Δ H - Δ (P V) = 44 - 14 = 30 L - a t m$
$x = 30 \times \frac{1}{10} = 3.$

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Q. One mole of a non ideal gas undergoes a change of state (

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Q. One mole of a non - ideal gas undergoes a change of state (2.0 atm, 3.0L, 95 K )

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Q. One mole of a non- ideal gas undergoes a change of state

(2.0 a t m, 3.0 L, 95 K) \to (4.0 a t m, 5.0 L, 245 K)

with a change in internal energy,

△ U = 30.0 L

atm. The change in enthalpy

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of the process is:

One mole of a non - ideal gas undergoes a change of state (2.0 atm, 3.0 L, 95K) $\to$ (4.0 atm, 5.0L, 245 K) with a change in internal energy $Δ U = 30.0 L$ atm. The change in enthalpy of the process in L atm is ?

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One mole of a non-ideal gas undergoes change of state (2.0 atm, 3.0 L, 95 K) → (4.0 atm, 5.0L, 245 K) with a change in enthalpy 44 L−atm. Calculate the change in internal energy (ΔU) in L−atm. Give the answer as x, where x=ΔU×110.

ΔU=ΔH−Δ(PV)=44−14=30L−atmx=30×110=3.

One mole of a non-ideal gas undergoes change of state (2.0 atm, 3.0 L, 95 K) $\to$ (4.0 atm, 5.0L, 245 K) with a change in enthalpy 44 L $-$ atm. Calculate the change in internal energy $(Δ U)$ in L $-$ atm. Give the answer as $x$ , where $x = Δ U \times \frac{1}{10} .$

$Δ U = Δ H - Δ (P V) = 44 - 14 = 30 L - a t m$
$x = 30 \times \frac{1}{10} = 3.$