What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0..8 bar and 2.0 L of O2 at 0.7 bar are introduced in a 1 L vessel at 27 °C ?

Question

What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0..8 bar and 2.0 L of O2 at 0.7 bar are introduced in a 1 L vessel at 27 °C ? (A) 1.8 bar (B) 2.8 bar (C) 3.0 bar (D) 5 bar

Tardigrade Admin · Accepted Answer

Partial pressure of hydrogen gas V1 = 0.5 L V2 = 1.0 L P1 =0.8 bar P2 = ? Applying Boyleâs law (constant T and n ) P1V1 = P2V2 or P2 =(P1V1/V2) ∴ P2 =((0.8 bar)×(0.5 L)/(1.0 L)) = 0.40 bar Partial pressure of oxygen gas, V1 = 2 .0 L, V2 = 1.0 L P1=0.7 bar P2 = ? or P2 = (P1V1/V2) =((0.7 bar)×(2.0 L)/(1.0 L)) = 1.40 bar Pressure of the gas mixture, Pmix = PH2+PO2=0.40+1.40 = 1.80 bar

Q. What will be the pressure of the gaseous mixture when 0.5L of H2​ at 0..8 bar and 2.0L of O2 at 0.7 bar are introduced in a 1L vessel at 27∘C?

1.8 bar

2.8 bar

3.0 bar

5 bar

Q. What will be the pressure of the gaseous mixture when $0.5 L$ of $H_{2}$ at $0..8$ bar and $2.0 L$ of $O 2$ at $0.7$ bar are introduced in a $1 L$ vessel at $27^{\circ} C$ ?