Compressed gases aren't ideal. Let's consider a gas that's non-ideal only because the volume available to each of the N molecules is reduced because each other molecule occupies volume v. Instead of pV=NkT, we get: p(V-Nb)=NkT. Let b=1.2 × 10-28 m3. Let's look at 3moles of this gas at T=300K starting in 0.001 m3 volume. 1) What's the initial value of the pressure?

P = 7482600 Pa = 7.482 MPa

Explanation:

We have the equation:

P(V - Nb) = NKT

here,

P = Initial Pressure = ?

V = Initial Volume = 0.001 m³

N = No. of moles = 3

b = constant = 1.2 x 10⁻²⁸ m³

T = Temperature = 300 k

k = Gas Constant = 8.314 J/mol . k

Therefore,

P[0.001 m³ - (3)(1.2 x 10⁻²⁸ m³)] = (3 mol)(8.314 J/mol. k)(300 k)

P = (7482.6 J)/(0.001 m³)

P = 7482600 Pa = 7.482 MPa

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c) up

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