calculate the pressure exerted by 1.00 moles of CO2 confined in a volume of 5.00 L at 450. K. Compare the pressure with that predicted by the ideal gas equation.
Something must be missing from your post. If you use PV = nRT, that IS the pressure predicted by ideal behavior. Perhaps you are to use the van der Waals equation and compare.
cap
To calculate the pressure exerted by 1.00 mole of CO2 confined in a volume of 5.00 L at 450 K, you can use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's calculate the pressure using the ideal gas law equation:
P = (nRT) / V
Given:
n = 1.00 mole
V = 5.00 L
T = 450 K
R = 0.0821 L·atm/(K·mol) (ideal gas constant)
Plugging in the values:
P = (1.00 mole * 0.0821 L·atm/(K·mol) * 450 K) / 5.00 L
P = 9.2766 atm
So, the pressure exerted by 1.00 mole of CO2 confined in a volume of 5.00 L at 450 K is approximately 9.28 atmospheres.
Now, let's compare this pressure with that predicted by the ideal gas equation. The ideal gas equation is:
PV = nRT
Since we are given the values of n, V, and T, we can rearrange the equation to solve for P:
P = (nRT) / V
Plugging in the values:
P = (1.00 mole * 0.0821 L·atm/(K·mol) * 450 K) / 5.00 L
P = 9.2766 atm
So, the pressure calculated using the ideal gas equation is the same as the pressure calculated using the ideal gas law equation. Therefore, they match each other.