Answer:
Total pressure = 16.42× 10⁻⁹atm
Explanation:
Given data:
Moles of H₂ = 2.50 × 10⁻³ mol
Moles of He = 1.00 × 10⁻³ mol
Mass of Ne = 3 × 10⁻⁴ mol
Volume = 10 L
Temperature = 35°C
Total pressure = ?
Solution:
Pressure of hydrogen:
P = nRT / V
P = 2.50 × 10⁻³ mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 308 K / 10 L
p = 63.22× 10⁻³ atm. L /10 L
P = 6.3 × 10⁻³atm
Pressure of helium:
P = nRT / V
P = 1.00 × 10⁻³ mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 308 K / 10 L
p = 25.29 × 10⁻³ atm. L /10 L
P = 2.53× 10⁻³ atm
Pressure of neon:
P = nRT / V
P = 3 × 10⁻⁴ mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 308 K / 10 L
p = 75.86× 10⁻³ atm. L /10 L
P = 7.59× 10⁻³ atm
Total pressure of mixture:
P(mixture) = pressure of hydrogen + pressure of helium+ pressure of neon
P(mixture) = 6.3 × 10⁻³atm + 2.53× 10⁻³ atm + 7.59× 10⁻³ atm
P(mixture) = 16.42× 10⁻⁹atm
If two plus two is four then four plus four is two
<span>CH3OH and NH3
I HOPE THIS HELPS :D</span>
