A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 moles of CO2 and 5.00 moles of N2 exerts a total pressure of 800 torr. What is the partial pressure?
Can you please includes steps on how to do this? So I will be able to do future problems!
2007-04-22 08:21:22 · 3 answers · asked by Azumi 2 in Science & Mathematics ➔ Chemistry
Okay so we know that partial pressures add to the total pressure. Luckily we're given the Total pressure. so the eqn looks like: PH2 + PNH3 + PCO2 + PN2 = TOTAL P
So lets use a formula and find the partials.
Partial P = (mole fraction ) x (total P)
ex. mole fraction for H2 would just be 2 moles of H2 divided by the total number of moles, 14 moles. Okay, now do u want your answer in atm or torr, I guess torr.
So, Partial of H2 = (2/14) x (800 torr) = 114.285 torr
partial of NH3 = (3/14) x (800) = 171. 428 torr
partial of CO2 = (4/14) x (800 ) = 228.571 torr
partial of N2 = (5/14) x (800) = 285.714 torr
and hey, when u add up those numbers we just got for the partials, bada bing bada boom, 800 torr. This isn't too bad. seeya hope this helped
2007-04-22 08:41:38 · answer #1 · answered by JoeyK 1 · 0⤊ 0⤋
Total moles = 14.
H2: (2/14) x 800
and so on.
2007-04-22 08:38:25 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
mole fractions are equal to pressure fractions, so your mole fraction of hydrogen will equal your pressure of hydrogen /800 torr and likewise for the rest.
2007-04-22 08:54:53 · answer #3 · answered by The Frontrunner 5 · 0⤊ 0⤋