5 mol of oxygen is heated at constant volume from 1 0 ∘ C to 2 0 ∘ C. Given C p = 8 cal/mol °C and R = 8.36 J/mol °C, the amount of heat consumed by oxygen is:

R = 4.18 8.36 = 2 cal/mol °C, so C v = 8 − 2 = 6 . Q = 5 × 6 × 10 = 300 cal. C.

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PhysicsHeat & ThermoThermodynamics Laws & Specific Heats of GasesMedium2 minQB

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5 mol of oxygen is heated at constant volume from $1 0^{\circ}$ C to $2 0^{\circ}$ C. Given $C_{p} = 8$ cal/mol °C and $R = 8.36$ J/mol °C, the amount of heat consumed by oxygen is:

Options:

Answer:

Solution:

$R = \frac{8.36}{4.18} = 2$ cal/mol °C, so $C_{v} = 8 - 2 = 6$ . $Q = 5 \times 6 \times 10 = 300$ cal. C.

Subject:PhysicsTopic:Heat & ThermoSubtopic:Thermodynamics Laws & Specific Heats of Gases

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