Question

One gram molecule of oxygen is heated at constant pressure from 0°C. What amount of heat should be imparted to the gas to double it's volume? Given cp = 0.218 cal g-1 0 C-1.

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Answer 1

Answer:

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n = 1

Oxygen is diatomic hence

Cp = (7/2)R Volume is doubled as constant pressure

∵ PV = nRT V = [(nRT) / P]

As P is constant, V ∝ T

Hence energy = Q = n CP ΔT = 1 × (7/2) × 8.31 × (2T1 – T1) = (7/2) × 8.31 × 2as T1 = 273K =

8000J = [(8000) / (4.18)]cal = 1911 cal

I hope it helps you !!

Answer 2

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n = 1

Oxygen is diatomic hence

Cp = (7/2)R Volume is doubled as constant pressure

∵ PV = nRT V = [(nRT) / P]

As P is constant, V ∝ T

Hence energy = Q = n CP ΔT = 1 × (7/2) × 8.31 × (2T1 – T1) = (7/2) × 8.31 × 2as T1 = 273K =

8000J = [(8000) / (4.18)]cal = 1911 cal