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The ideal pressure of 0.30 mol of He in 0.20 L is 30.55 atm at -25°C. What is the real gas pressure?

User Greg Bala
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1 Answer

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To determine the real gas pressure, we need to apply the ideal gas law equation:

PV = nRT

Where:

P = pressure

V = volume

n = number of moles

R = ideal gas constant

T = temperature

Given:

Number of moles (n) = 0.30 mol

Volume (V) = 0.20 L

Temperature (T) = -25°C (converted to Kelvin: -25°C + 273.15 = 248.15 K)

The ideal gas constant (R) is a constant value of 0.0821 L·atm/mol·K.

Substituting the values into the equation:

P * 0.20 L = 0.30 mol * 0.0821 L·atm/mol·K * 248.15 K

Simplifying the equation:

P * 0.20 L = 0.30 mol * 20.307 L·atm

P = (0.30 mol * 20.307 L·atm) / 0.20 L

P = 6.0921 atm

Therefore, the real gas pressure is 6.0921 atm.

User Ronaldosantana
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