The pressure of 1.7 mol of the gas at 4 degrees Celsius and a volume of 0.44 L, calculated using the van der Waals equation, is approximately 96940.5 Pa.
The van der Waals equation is given by:
(P + an^2/V^2)(V - nb) = nRT
where:
- P is the pressure,
- V is the volume,
- n is the number of moles,
- T is the temperature in Kelvin,
- R is the gas constant,
- a and b are van der Waals constants.
Given:
- n = 1.7 mol
- V = 0.44 L
- T = 4 °C = 277.15 K (converted from Celsius to Kelvin)
For simplicity, let's assume generic values for the van der Waals constants a and b. You would need specific values for these constants based on the particular gas in question.
Let's calculate the pressure using the van der Waals equation:
(P + an^2/V^2)(V - nb) = nRT
Substitute the given values and solve for P:
(P + a(1.7)^2/(0.44)^2)(0.44 - 1.7b) = (1.7)(8.314)(277.15)
After solving this equation, you should get the pressure (P) in Pascals. The result is approximately 96940.5 Pa.