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Chemistry - Thermodynamics - I Question with Solution | TestHub

ChemistryThermodynamics - IHeat & Heat CapacityMedium2 minQB

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Calculate change in internal energy for 2 moles of an ideal gas when temperature rises from 27°C to 127°.

Given: $C_{p, m} (J K^{- 1} m o l^{- 1}) = 13.314 + 0.04 T$

Options:

Answer:

Solution:

$C_{v, m} = C_{p, m} - R \Rightarrow (13.314 - 8.314) + 0.04 T \Rightarrow 5 + 0.04 T$

$Δ U = n . C_{v, m} .Δ T$

$Δ U = (\int_{T_{1}}^{T_{2}} (5 + 0.04 T)) \times 2$

$Δ U = (5 (Δ T) + 0.4 (\frac{T _{2}^{2}}{2} - \frac{T _{1}^{2}}{2})) \times 2$ $Δ U = (5 \times 100 + \frac{0.04}{2} (160000 - 90000)) \times 2 = 3800 J$

Stream:JEESubject:ChemistryTopic:Thermodynamics - ISubtopic:Heat & Heat Capacity

⏱ 2mℹ️ Source: QB

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