Question

Two flasks are connected with a stopcock. flask #1 has a volume of 2.5 l and contains

oxygen gas at a pressure of 0.70 atm. flask #2 has a volume of 3.8 l and contains
hydrogen gas at a pressure of 1.25 atm. when the stopcock between the two flasks is
opened and the gases are allowed to mix, what will the resulting pressure of the gas
mixture be?
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Answer 1

Okay, let's solve this step-by-step:

* Flask 1 has volume 2.5 L and pressure 0.7 atm of oxygen gas

* Flask 2 has volume 3.8 L and pressure 1.25 atm of hydrogen gas

When the stopcock is opened and the gases mix, they will occupy the total volume of both flasks, which is 2.5 L + 3.8 L = 6.3 L.

We can use the ideal gas law, PV = nRT, to find the final pressure. Since the amount of gas (n) and temperature (T) do not change, P and V are inversely proportional.

So the final pressure will be:

Initial pressure of flask 1 * (volume of flask 1/ total volume) +

Initial pressure of flask 2 * (volume of flask 2/ total volume)

= (0.7 atm * (2.5 L/6.3 L)) + (1.25 atm * (3.8 L / 6.3 L))

= 0.44 atm + 0.81 atm

= 1.25 atm

So the final pressure of the gas mixture will be 1.25 atm.