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
Question
Question
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
Answer:
The partial pressure of H2 is 0.375 atm
The partial pressure of Ne is also 0.375 atm
Explanation:
Mass of H2 = 1 g
Mass of Ne = 1 g
Mass of Ar = 1 g
Mass of Kr = 1 g
Total mass of gas mixture = 1 + 1 + 1 + 1 = 4 g
Pressure of sealed container = 1.5 atm
Partial pressure of H2 = (mass of H2/total mass of gas mixture) × pressure of sealed container = 1/4 × 1.5 = 0.375 atm
Partial pressure of Ne = (mass of Ne/total mass of gas mixture) × pressure of sealed container = 1/4 × 1.5 = 0.375 atm