Chemistry
posted by Kayla on .
Bulb A is 100mL and contains Helium at 1atm.
Bulb B is 500ml and contains Argon at 2atm
The bulbs are connected together by a valve.
(assume constant temperature).
What is the total pressure of the system after the valves are opened?

The long way to do this, but the easier way to explain, is this.
Use PV = nRT for bulb A and solve for n = mols He.
Then use PV = nRT for bulb B and solve for n = mols Ar.
Add n He + n Ar = total n
Then PV = nRT. Use total n and solve for P. (Note: you don't have a T listed so just use a convenient one but don't change it) 
Would the total pressure be 2.19985 atm? Could you possibly help me with this one?

No, that isn't right.
What's the problem with plugging in the numbers? For example, for He, you can use
PV = nRT.
n = PV/RT
n = 1*0.1/(0.08206*300)
n = 0.00406
For Ar.
n = PV/RT = 2*0.500/(0.08206*300)
n = 0.406
Total n = 0.0406+0.00406 = 0.0446
Then p = nRT/V = 0.41*0.08206*300/0.600
P = ?
You can also do this a much shorter way by using P1V1 = P2V2
For He that is P2 = P1V1/V2
P2 He = 1*(100/600) = 0.167
P2 Ar = 2*(500/600) = 1.67
Total P = 0.167+1.67 = ?