Given data,
n=number of moles (Assume n=1)
P=Pressure (atm)
V=Volume (L) (0.065 <= V <=1)
T=Temperature (Assume T = 20C = 293K)
R=Gas constant = 0.08206 (L atm )/(mol K)
For CO2 ,
a = L2 atm / mol2
b = 0.04267 L/mol
Put all values in MATLAB command (define variables as given above)
>> n=1;R=0.08206;T=293;V=[0.065:0.005:1];
>> a=3.592;b=0.04267; %CO2 properties
>> P=(n*R*T)./V; % Ideal gas equation
>> Pw=((n*R*T)./(V-n*b))-((n^2*a)./(V.^2)); % Real gas equation
>> plot(V,P,'r',V,Pw,'k','LineWidth',2)
>> grid on
>> xlabel('Volume (L)');
>> ylabel('Pressure (atm)');
>> legend('Ideal Gas Eqaution','van der Waals Equation')
This will return a plot as shown in figure
Code to Matlab Make two plots on one page. mo ad tle veloclty as a function...
The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles (n): PV=nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van...
Consider example 14.1. What is the ratio of the mass of a single
molecule of the ideal gas in the example, to its (molecular
velocity)2? Be sure that you're using the correct units and to
include R in your function. (Hint: Your answer should be m/u2 =
??)
535 One mole of an ideal gas at 0°C and 1.00 atm pressure contains 6.022 x 10 molecules (Avogadro's number) and occupies a volume of 22.414 L. A good States of Matter...