What will be the pressure of the gaseous mixture when 0.5 L of H₂ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?

Question

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 dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?

Philoid · Accepted Answer

Let the partial pressure of hydrogen in the vessel be P_a.

P₁ = 0.8 bar,

V₁ = 0.5L

V₂ = 1L

P₂ = P_a

Now, at constant temperature

⇒ P₁V₁ = P₂V₂

⇒

P_a = 0.4 bar

Similarly, for oxygen we get the partial pressures of oxygen as

⇒

⇒ P_b = 1.4 bar

It is known that,

The total pressure exerted is the sum of partial pressures so total pressure is (1.4+0.4) = 1.8 bar.

What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?