The total pressure of the gases in the vessel is found out by using the partial pressures of individual gases and adding them up. The total pressure of the gases in the vessel is 1.72 atm.
The Partial pressure of the gases is the individual pressure of the gases present in a vessel containing a mixture of gases. The total pressure can be found out by adding partial pressure of all gases.
Given:
Volume of vessel, V= 32.5L
Mass of Nitrogen gas = 2.8g
Mass of Hydrogen gas = 0.403g
Mass of Argon gas = 79.9g
We know that:
Molar Mass of Nitrogen gas = 28g
Molar Mass of Hydrogen gas = 2g
Molar Mass of Argon gas = 40g
∴ Moles of gas = Given mass / Molar mass
∴ Using the Ideal Gas Equation:
PV = nRT
where, P is the Pressure of gas
V is the volume of gas
n is the moles of gas
R is the Universal Gas constant
T is the temperature
Applying the above equation of all three gases indivudually,
∴ For Nitrogen,
P₁V = n₁RT
⇒ P₁ × 32.5 = 2.8/28 × 0.082 × 298
⇒ P₁ = 0.07atm
∴ For Hydrogen,
P₂V = n₂RT
⇒ P₂ × 32.5 = 0.4/2 × 0.082 × 298
⇒ P₂ = 0.15 atm
∴ For Argon,
P₃V = n₃RT
⇒ P₃ × 32.5 = 79.9/40 × 0.082 × 298
⇒ P₃ = 1.5 atm
∴ Total pressure of vessel, P = P₁ + P₂ + P₃
P = 1.72 atm
The total pressure of the gases in the vessel is 1.72 atm.
Learn more about Partial pressure here, brainly.com/question/23841760
#SPJ4
