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
    
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