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:
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
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Answered by
8
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
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