Question
A gaseous mixture of O2, H2, and N2 has a total pressure of 1.50 atm and contains 8.20 g
of each gas. Find the partial pressure of each gas in the mixture
They don't give you Volume and Temperature. Please explain it to me, thank you!
of each gas. Find the partial pressure of each gas in the mixture
They don't give you Volume and Temperature. Please explain it to me, thank you!
Answers
You want to convert 8.2 g O2 to moles, 8.2 g N2 to moles, 8.2 g H2 to moles.
Then determine the mole fraction of each.
partial pressure each = Xof each*1.5 atm.
moles fraction, O2 for example, = moles O2/total number of moles.
Then determine the mole fraction of each.
partial pressure each = Xof each*1.5 atm.
moles fraction, O2 for example, = moles O2/total number of moles.
Related Questions
A gaseous mixture at a total pressure of 1.50 atm contains equal molar amounts of He, Ne, and Ar. At...
A gaseous mixture of and contains 30.8 nitrogen by mass. What is the partial pressure of oxygen i...
a gaseous mixture contains 1 mol of O2 and 2 mol of CO2, exerting a total pressure of 1.5 atm. what...
A gaseous mixture was prepared by taking equal mole of CO and N2 .if the total pressure of the mixtu...