A mixture consists of 3.2 grams of CH4 gas and 1.2 grams of H2 in a steel container. The pressure inside the container is 6.0 atm. The molecular mass of CH4 is 16 g/mol, and the molecular mass of H2 gas is 2 g/mol.
What is the partial pressure of H2?
4.5 atm
moles CH4=3.2/16=.2
moles H2=1.2/2=.6
mole ratio CH4/H2=1/3
so the pressure is 6atm, consisting of four parts, three of which are H2, and one which is CH4
PressureH2=6*3/4=4.5atm
PressureCH4=6*1/4=1.5atm
those are the partial pressures.
To find the partial pressure of H2, you can use the concept of mole fraction. The mole fraction of a component is the ratio of the number of moles of that component to the total number of moles in the mixture.
Let's calculate the number of moles of each component first:
Number of moles of CH4 = Mass of CH4 / Molecular mass of CH4
= 3.2 g / 16 g/mol
= 0.2 mol
Number of moles of H2 = Mass of H2 / Molecular mass of H2
= 1.2 g / 2 g/mol
= 0.6 mol
The total number of moles in the mixture is the sum of the moles of CH4 and H2:
Total moles = Moles of CH4 + Moles of H2
= 0.2 mol + 0.6 mol
= 0.8 mol
Now, we can calculate the mole fraction of H2:
Mole fraction of H2 = Moles of H2 / Total moles
= 0.6 mol / 0.8 mol
= 0.75
Finally, to find the partial pressure of H2, we multiply the mole fraction by the total pressure:
Partial pressure of H2 = Mole fraction of H2 × Total pressure
= 0.75 × 6.0 atm
= 4.5 atm
Therefore, the partial pressure of H2 is 4.5 atm.
To find the partial pressure of H2 in the mixture, we need to use the concept of mole fraction.
The first step is to calculate the number of moles of each gas present in the mixture.
1. Moles of CH4:
- Number of moles = mass / molar mass
- Moles of CH4 = 3.2 g / 16 g/mol = 0.2 mol
2. Moles of H2:
- Number of moles = mass / molar mass
- Moles of H2 = 1.2 g / 2 g/mol = 0.6 mol
Next, we find the total number of moles of both gases:
Total moles = moles of CH4 + moles of H2
Total moles = 0.2 mol + 0.6 mol
Total moles = 0.8 mol
Now, we calculate the mole fraction of H2:
Mole fraction of H2 = Moles of H2 / Total moles
Mole fraction of H2 = 0.6 mol / 0.8 mol
Mole fraction of H2 = 0.75
Finally, we use the mole fraction to find the partial pressure of H2:
Partial pressure of H2 = Mole fraction of H2 * Total pressure
Partial pressure of H2 = 0.75 * 6.0 atm
Partial pressure of H2 = 4.5 atm
Therefore, the partial pressure of H2 in the mixture is 4.5 atm.