Asked by ZMD
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.
atm and the total pressure in the flask is
atm.
Answers
Answered by
DrBob222
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.
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.
Answered by
DrBob222
Sorry but I made a typo on R by leaving out a decimal. R is 0.08206