mols = grams/atomic mass
mols Kr = 13.5/atomic mass Kr = ?
mols N2 = 3.04/molar mass N2 = ?
P = nRT
for partial pressure Kr plug in mols Kr for n and the T listed. R is 008206. Solve for P.
Do the same for partial pressure N2 but use mols N2 for n.
For total P just add them; i.e., Ptotal = PN2 + PKr
Post your work if you get stuck.
A mixture of nitrogen and krypton gases, in a 6.51 L flask at 84 °C, contains 3.04 grams of nitrogen and 13.5 grams of krypton. The partial pressure of krypton in the flask is
atm and the total pressure in the flask is
atm.
2 answers
Sorry but I made a typo on R by leaving out a decimal. R is 0.08206