Question #c8a2e
1 Answer
Explanation:
The idea here is that you can use Dalton's law of partial pressures to help you find a relationship between the total pressure of gaseous mixture and the partial pressure of
Now, the mole percent of a gas that's part of a gaseous mixture is simply the mole fraction of that gas multiplied by
#color(blue)("mole%" = chi xx 100)" "# , where
This means that you can use the mole percent of gas
#"mole %" = chi x 100 implies chi = "mole %"/100#
Therefore, you have
#chi_"A" = 10/100 = 0.1#
Since the mixture only contains two gases,
#chi_"A" + chi_"B" = 1#
This means that the mole fraction of
#chi_"B" = 1 - 0.1 = 0.9#
Now, STP conditions are usually given as a pressure of
SIDE NOTE I say usually because the actual conditions for STP are a pressure of
Dalton's law of partial pressures tells you that the partial pressure of each component of a gaseous mixture is proportional to that component's mole fraction.
The total pressure of the mixture can thus be written as
#P_"total" = overbrace(chi_"A" xx P_"total")^(color(red)("partial pressure of A")) + overbrace(chi_"B" xx P_"total")^(color(blue)("partial pressure of B"))#
This means that the partial pressure of
#P_"B" = chi_"B" xx P_"total"#
#P_"B" = 0.9 * "1 atm" = color(green)("0.9 atm")#
You can read more on mole percent and mole fraction here: