A ﬂask contains a gas mixture of methane, hydrogen. and nitrogen with partial pressures of 1 atm. 1.2 atm, and 1.1 aim, respectively. What is the total pressure of the mixture?

Oct 30, 2015

$\text{3.3 atm}$

Explanation:

The idea here is that you can use Dalton's Law of Partial Pressures to express the total pressure of the gaseous mixture as the sum of the partial pressures of the individual components of the mixture.

color(blue)(P_"total" = sum_i (P_"partial i")) " ", where

${P}_{\text{partial i}}$ - the partial pressure of component $i$
${P}_{\text{total}}$ - the total pressure of the mixture In your case, you know that the mixture contains three gases, methane, hydrogen, and nitrogen, each with its own partial pressure

• $\text{CH"_4 -> "1.0 atm}$
• $\text{H"_2 -> "1.2 atm}$
• $\text{N"_2 -> "1.1 atm}$

This means that the total pressure of the mixture will be

${P}_{\text{total}} = {P}_{C {H}_{4}} + {P}_{{H}_{2}} + {P}_{{N}_{2}}$

P_"total" = "1.0 atm" + "1.2 atm" + "1.1 atm" = color(green)("3.3 atm")

The underlying principle that's at work here is the fact that at constant temperature and volume, the pressure of a gas is proportional ot the number of moles of gas.