Question #1cee1
1 Answer
Explanation:
The idea here is that you can determine the partial pressure of argon by using Dalton's Law of Partial Pressures, which states that the partial pressure of a gas
#color(blue)(|bar(ul(color(white)(a/a)P_i = chi_i xx P_"total"color(white)(a/a)|)))#
Here
Now, you know that argon makes up
Since volume is directly proportional to number of moles at constant temperature and pressure -- think Avogadro's Law here -- you can say that you have
This means that the mole fraction of argon, which is defined as the ratio between the number of moles of argon and the *total number of moles8 of gas present in a given sample of air, will be
#chi_"argon" = (0.93 color(red)(cancel(color(black)("moles"))))/(100color(red)(cancel(color(black)("moles")))) = 0.0093#
The partial pressure of argon in air will be
#P_"argon" = 0.0093 * "760 mmHg" = color(green)(|bar(ul(color(white)(a/a)color(black)("7.07 mmHg")color(white)(a/a)|)))#
I'll leave the answer rounded to three sig figs.