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.