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 = ?

To find the total pressure of the system after the valves are opened, we need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature

Since the temperature is assumed to be constant, we can combine the two bulbs into one system by adding their volumes and pressures:

V_total = V_A + V_B = 100 mL + 500 mL = 600 mL

P_total = n_total * R * T / V_total

To simplify the equation, we can assume that the moles of gas in each bulb are negligible compared to the combined system. This is a reasonable assumption if the initial volumes of gas are small relative to the total volume of the system. Therefore, we can disregard the moles of gas term (n_total) in the equation.

P_total = R * T / V_total

Now, we know the volumes of the bulbs and the pressures in each of them. However, we also need to convert the volumes to liters and pressures to atmospheres since the values we have are currently in milliliters and atmospheres, respectively.

Converting V_total to liters:
V_total = 600 mL * 1 L / 1000 mL = 0.6 L

Using the pressure-volume equivalence, we can convert the pressure of each bulb to atmospheres:
1 atm = 101.325 kPa ≈ 101.325 J/L

Converting P_A to atmospheres:
P_A = 1 atm * (101.325 J/L) / 1 atm = 101.325 J/L

Converting P_B to atmospheres:
P_B = 2 atm * (101.325 J/L) / 1 atm = 202.65 J/L

Substituting these values into the equation, we get:

P_total = R * T / V_total
P_total = (0.0821 L*atm/(mol*K)) * T / 0.6 L

As we don't have the temperature (T) in the question, we need to assume a value for it to calculate the result. Once we have the temperature, we can plug it into the equation to find the total pressure of the system.