calculate the pressure exerted by 2.50 moles of CO2 confined in a volume of 5.00 L at 450K. Compare the pressure with that predicted by the ideal gas equation.
so the answer would be18.5 atm using the formula p= nRt/V correct?
18.5 atm is the pressure calculated as an ideal gas. I have no idea what you are to compare it with.
To calculate the pressure exerted by 2.50 moles of CO2 in a volume of 5.00 L at 450K, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal Gas Constant (0.0821 L·atm/mol·K)
T = Temperature
Let's plug in the values:
P * 5.00 L = 2.50 mol * 0.0821 L·atm/mol·K * 450K
5.00P = 102.625
Now, we can solve for P:
P = 102.625 / 5.00
P ≈ 20.53 atm
Therefore, the pressure exerted by 2.50 moles of CO2 in a volume of 5.00 L at 450K is approximately 20.53 atm.
Now let's compare this pressure with that predicted by the ideal gas equation. The ideal gas equation predicts the pressure based on assuming that gases behave ideally, which means that there are no intermolecular forces and the volume of the molecules themselves is negligible compared to the volume of the container. Therefore, in ideal conditions, we expect the predicted pressure to be the same as the calculated pressure.
So, in this case, the pressure calculated using the Ideal Gas Law is the same as the pressure predicted by the ideal gas equation.
To calculate the pressure exerted by the gas, we can use the ideal gas equation, which is given by:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(K·mol))
T = temperature (in Kelvin)
Let's plug in the values:
n = 2.50 moles
V = 5.00 L
T = 450 K
R = 0.0821 L·atm/(K·mol)
Using the above equation, we can solve for P:
P = (nRT) / V
P = (2.50 moles * 0.0821 L·atm/(K·mol) * 450 K) / 5.00 L
P ≈ 73.725 atm
Therefore, the pressure exerted by 2.50 moles of CO2 confined in a volume of 5.00 L at 450K is approximately 73.725 atm.
To compare this pressure with that predicted by the ideal gas equation, we can calculate the pressure using the ideal gas equation with the same values of n, V, and T:
P = (nRT) / V
P = (2.50 moles * 0.0821 L·atm/(K·mol) * 450 K) / 5.00 L
P ≈ 73.725 atm
The pressure calculated using the ideal gas equation is also approximately 73.725 atm. Therefore, the pressure predicted by the ideal gas equation matches the pressure calculated for this case.