Three gases (8.00 of methane, 18.0 of ethane, and an unknown amount of propane, were added to the same 10.0-L container. At 23.0 C , the total pressure in the container is 3.60 atm. Calculate the partial pressure of each gas in the container.
Use PV = nRT and calculate pressure for methane. Convert 8.00 (WHAT) to moles.
Do the same for 18.0 WHAT ethane.
Then partial pressure CH4 + partial pressure ethane + partial pressure unknown = 3 atm.
16
Take your methane first. Find the moles by dividing the mass (8.00g) by the molar mass (which can be found by the chemical formuls CH4 = 16.042g/mol). Then you can rearrange the ideal gas formula to solve for the pressure of methane (P=nRT/V). This is your partial pressure for methane! You can do the same thing for ethane which has a chemical formula of C2H6. To solve for the partial pressure of the unknown gas you can use the formula: Ptotal=Pmethane+Pethane+Punknown... Your Ptotal is given as 3.60atm so just rearrange and for your unknown partial pressure. Hope this helps anyone else who needed this information!! :)
For anyone on Mastering Chemistry, I got the final answer as methane: 1.21atm, ethane: 1.45atm, and unknown: 0.940atm.
I got the final answer as methane: 1.21atm, ethane: 1.45atm, and unknown: 1.940atm.
To calculate the partial pressure of each gas in the container, we can use Dalton's law of partial pressures. According to Dalton's law, the total pressure of a gaseous mixture is equal to the sum of the partial pressures of each gas in the mixture.
Step 1: Convert the given masses of each gas to moles.
The molar mass of methane (CH4) is 16.04 g/mol.
Number of moles of methane = mass of methane / molar mass of methane
= 8.00 g / 16.04 g/mol
≈ 0.499 mol
The molar mass of ethane (C2H6) is 30.07 g/mol.
Number of moles of ethane = mass of ethane / molar mass of ethane
= 18.0 g / 30.07 g/mol
≈ 0.598 mol
We don't have the mass of propane, but we can use the ideal gas law to find the number of moles of propane. The ideal gas law is given by the 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.
Step 2: Convert the given total pressure to Kelvin.
Temperature in Kelvin = 23.0 °C + 273.15 = 296.15 K
Step 3: Use the ideal gas law to find the number of moles of propane.
(3.60 atm) * (10.0 L) = n(propane) * (0.0821 L.atm/mol.K) * (296.15 K)
n(propane) ≈ (3.60 atm * 10.0 L) / (0.0821 L.atm/mol.K * 296.15 K)
≈ 0.488 mol
Step 4: Calculate the partial pressure of each gas.
Total moles of gases = moles of methane + moles of ethane + moles of propane
≈ 0.499 mol + 0.598 mol + 0.488 mol
≈ 1.585 mol
Partial pressure of methane = (moles of methane / total moles of gases) * total pressure
≈ (0.499 mol / 1.585 mol) * 3.60 atm
≈ 1.135 atm
Partial pressure of ethane = (moles of ethane / total moles of gases) * total pressure
≈ (0.598 mol / 1.585 mol) * 3.60 atm
≈ 1.357 atm
Partial pressure of propane = (moles of propane / total moles of gases) * total pressure
≈ (0.488 mol / 1.585 mol) * 3.60 atm
≈ 1.108 atm
So, the partial pressure of methane, ethane, and propane in the container are approximately 1.135 atm, 1.357 atm, and 1.108 atm, respectively.