Approximately 1.000 g each of four gasses H2, Ne, Ar, and Kr are placed in a sealed container all under1.5 atm of pressure. Assuming ideal behavior, determine the partial pressure of the H2 and Ne?
To determine the partial pressure of H2 and Ne, we can first calculate the mole fraction of each gas and then use it to find the partial pressure.
1. Calculate the moles of each gas:
- For H2:
1.000 g H2 * (1 mol H2 / 2.01588 g H2) = 0.4962 mol H2
- For Ne:
1.000 g Ne * (1 mol Ne / 20.1797 g Ne) = 0.0495 mol Ne
2. Calculate the total moles:
Total moles = moles of H2 + moles of Ne + moles of Ar + moles of Kr
Total moles = 0.4962 mol + 0.0495 mol + 0.0495 mol + 0.0495 mol = 0.6447 mol
3. Calculate the mole fraction of each gas:
- For H2:
X_H2 = moles of H2 / total moles
X_H2 = 0.4962 mol / 0.6447 mol = 0.7693
- For Ne:
X_Ne = moles of Ne / total moles
X_Ne = 0.0495 mol / 0.6447 mol = 0.0768
4. Calculate the partial pressure:
- For H2:
P_H2 = X_H2 * total pressure
P_H2 = 0.7693 * 1.5 atm = 1.1539 atm
- For Ne:
P_Ne = X_Ne * total pressure
P_Ne = 0.0768 * 1.5 atm = 0.1152 atm
Therefore, the partial pressure of H2 is 1.1539 atm and the partial pressure of Ne is 0.1152 atm.