a correction needs to be made to the calculations for real gases as compared to ideal gases. apply these corrections and calculate the real pressure expected for 5 mole of nitrogen in a 1.5L container at a temp. of 20C.
Note: I tried to find right formula for this but couldnt. so i really need help with this now!!!!
Look in your text for the van der Waals equation for gases. Here is a link on the web if you have trouble finding it in your text.
http://en.wikipedia.org/wiki/Van_der_Waals_equation
Thank you sooooooooo much!!!!!!
Here is a link for the constants a and b in the van der Waals equation.
http://en.wikipedia.org/wiki/Van_der_Waals_constants_%28data_page%29
To calculate the real pressure of a gas using corrections for real gases, we will need to use the Van der Waals equation, which is an improvement on the ideal gas law. The Van der Waals equation accounts for the volume and attractive forces between gas particles.
The Van der Waals equation is as follows:
(P + a(n^2/V^2))(V - nb) = nRT
Where:
P = real pressure
n = the number of moles of gas
V = volume of the container
T = temperature in Kelvin
a = intermolecular attraction constant
b = molecular size constant
R = ideal gas constant (0.0821 L.atm/mol.K)
To begin, let's convert the given temperature of 20°C to Kelvin:
T = 20 + 273.15 = 293.15 K
The intermolecular attraction constant (a) and molecular size constant (b) values depend on the specific gas. For nitrogen gas (N2), these values are approximately:
a = 1.39 atm.L^2/mol^2
b = 0.0391 L/mol
Now, we can substitute the values into the Van der Waals equation and solve for the real pressure (P) of nitrogen in the given conditions:
(P + (1.39 * (5^2/1.5^2)))(1.5 - (0.0391 * 5)) = 5 * 0.0821 * 293.15
Simplifying this equation will give you the value for the real pressure of nitrogen in the 1.5L container at a temperature of 20°C.