Using the information on the table of van der Waals Constants of Some Common gases, calculate the pressure exerted by 4.37 moles of chlorine gas confined in a volume of 2.45 L at 38 degrees Celsius. Compare the pressure with that calculated using the ideal gas equation.
See your other post above.
To calculate the pressure exerted by chlorine gas using the van der Waals equation, we need the van der Waals constants for chlorine gas. Unfortunately, you mentioned a "table of van der Waals constants of Some Common gases," but did not provide the specific van der Waals constants for chlorine gas. Therefore, I cannot give you an exact calculation using the van der Waals equation.
However, I can guide you through the process of using the ideal gas equation to calculate the pressure of the chlorine gas. The ideal gas equation is given by:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, we need to convert the given temperature of 38 degrees Celsius to Kelvin by adding 273.15:
T = 38 + 273.15 = 311.15 K
Next, we can substitute the given values into the ideal gas equation:
P * 2.45 = 4.37 * 0.0821 * 311.15
Solving this equation will give you the pressure in atm.
Now, to compare this pressure with that calculated using the van der Waals equation, you would need the specific van der Waals constants for chlorine gas. With those values, you can use the van der Waals equation:
(P + a(n/V)^2) * (V - nb) = nRT
Where:
a and b are the van der Waals constants specific to the gas.
You can substitute the given values and calculate the pressure using the van der Waals equation. Then, compare the results obtained from both equations to see the difference in pressure calculations.
Please note that the van der Waals equation takes into account the molecular interactions and the finite volume of gas particles, unlike the ideal gas equation, which assumes no molecular interactions and zero particle volume.