Determine the number of moles of Krypton contained in a 3.25 liter gas tank at 5.80 bar and 25.5 °C. If the gas were Oxygen instead of Krypton, how will the answer change? Explain.
Use PV = nRT and solve for n. Remember to use kelvin for T; i.e., K = 273.2 + 25.5 C = ?
For the second part with oxygen just substitute the different values.
Post your work if you get stuck.
To determine the number of moles of Krypton contained in the gas tank, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the given values to Kelvin and atmospheres:
Pressure:
5.80 bar can be converted to atmospheres using the conversion factor 1 bar = 0.9869 atm.
So, 5.80 bar is approximately 5.725 atm.
Temperature:
25.5 °C needs to be converted to Kelvin by adding 273.15:
T = 25.5 °C + 273.15 = 298.65 K
Now we can plug the values into the ideal gas law equation and solve for the number of moles (n):
P * V = n * R * T
n = (P * V) / (R * T)
n = (5.725 atm * 3.25 L) / (0.0821 L·atm/(mol·K) * 298.65 K)
n ≈ 0.318 moles of Krypton
If the gas were Oxygen instead of Krypton, the answer would change because the molar mass of Oxygen is different from that of Krypton. Oxygen has a molar mass of about 32 g/mol, while Krypton has a molar mass of about 83.8 g/mol.
So, to calculate the number of moles of Oxygen, we can use the molar mass and the mass of Oxygen in the tank. However, since the mass of Oxygen is not provided in the question, we cannot determine the number of moles of Oxygen without more information.
In conclusion, the answer would change since the molar mass of Oxygen is different from that of Krypton.
To determine the number of moles of Krypton in the gas tank, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in Pascal
V = volume in cubic meters
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature in Kelvin
First, we need to convert the given values to the correct units:
Pressure:
5.80 bar = 580,000 Pascal (since 1 bar = 100,000 Pascal)
Volume:
3.25 liters = 0.00325 cubic meters (since 1 liter = 0.001 cubic meters)
Temperature:
25.5 °C = 298.65 K (since 0 °C = 273.15 K)
Now, we can plug in the values into the ideal gas law equation:
580,000 Pascal * 0.00325 cubic meters = n * 8.314 J/(mol·K) * 298.65 K
Solving for n, we get:
n = (580,000 * 0.00325) / (8.314 * 298.65)
n ≈ 0.0807 moles
Therefore, there are approximately 0.0807 moles of Krypton in the gas tank.
If the gas were Oxygen instead of Krypton, the answer would change because the molar mass of Oxygen and Krypton are different. Oxygen has a molar mass of approximately 32.00 g/mol, while Krypton has a molar mass of approximately 83.80 g/mol.
To find the number of moles of Oxygen, we would need the mass of the gas and divide it by the molar mass of Oxygen (remembering to convert the mass to grams if necessary). The ideal gas law equation would remain the same, but the molar mass value would be different.
In summary, the answer would change because the molar mass of Oxygen is different from Krypton, resulting in a different number of moles in the gas tank.