A 260-mL flask contains pure helium at a pressure of 743 torr. A second flask with a volume of 480 mL contains pure argon at a pressure of 715 torr.

If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of helium? in torr

If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of argon? in torr

If the two flasks are connected through a stopcock and the stopcock is opened, what is the total pressure? in torr

Well, aren't these flasks just a great match for each other! It's like the helium and argon are having a little party in there. Let me crunch some numbers for you.

To find the partial pressure of helium, we need to consider its initial pressure and volume. Since helium is in the first flask, its partial pressure will remain the same as the initial pressure, which is 743 torr.

Now, let's move on to the argon in the second flask. Similarly, its partial pressure will also remain the same as the initial pressure, which is 715 torr.

Now, let's talk about the total pressure. When the two flasks are connected, the gases will mix together, just like a DJ mixing beats at a party. The total pressure will be the sum of the partial pressures of helium and argon. So, the total pressure will be 743 torr + 715 torr, which gives us a grand total of 1458 torr.

So, to sum it up:

Partial pressure of helium: 743 torr
Partial pressure of argon: 715 torr
Total pressure: 1458 torr

Now let's just hope the helium and argon don't start arguing about who gets to be at the top of the flask!

To find the partial pressure of helium when the two flasks are connected, we need to consider Dalton's Law of Partial Pressures. According to this law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.

1. To find the partial pressure of helium:
- Given: Volume of helium flask (V₁) = 260 mL, Helium pressure (P₁) = 743 torr
- Use the equation: P₁V₁ = P_total * V_total
- Since the stopcock is opened, the total volume (V_total) is the sum of the volumes of both flasks, which is 260 mL + 480 mL = 740 mL
- Rearranging the equation, we get: P_total = (P₁V₁) / V_total
- Substituting the values, P_total = (743 torr * 260 mL) / 740 mL

2. To find the partial pressure of argon:
- Given: Volume of argon flask (V₂) = 480 mL, Argon pressure (P₂) = 715 torr
- Since the stopcock is opened, the total volume (V_total) is still 740 mL.
- Using the same equation, P_total = (P₂V₂) / V_total, we can find the partial pressure of argon.

3. To find the total pressure:
- The total pressure is simply the sum of the partial pressures of helium and argon, which can be calculated by adding the results from the previous steps.

By following these steps, you can calculate the partial pressures of helium and argon, as well as the total pressure in the system.

I assume they are both at the same temperature initially.

Parial pressure is dependent on mole ratio. n=PV/RT in each flask, find n for each first.
Then ADD the n for each. That is the N for the combined.
PV=NRT now solve for P for the combined gases.

Parg+Phelium= P
Parg=narg/N * P
Phelium= nhelium/N* P

752 torr of He

582 torr of Ar
total=1334 torr