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The stopcock connecting a 1.88 L bulb containing xenon gas at a pressure of 8.40 atm, and a 9.20 L bulb containing oxygen gas at a pressure of 3.99 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is atm?

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Answer:

Final pressure is 4.73 atm

Explanation:

In a mixture of gases:

Total pressure = Sum of partial pressure of each gas

Total moles = Sum of moles of each gas

We assume additives volume → 1.88L + 9.20L = 11.08L

Let's apply the Ideal Gases Law to determine the moles of Xe and O₂

P . V = n. R . T → (P. V / R . T) = n

8.40atm . 1.88L / 0.082 . 273K = n → 0.70 moles of Xe

3.99atm . 9.20L / 0.082 . 273K = n → 1.64 moles of O₂

Total moles = 0.70 moles of Xe + 1.64 moles of O₂ → 2.34 moles

P = (n . R . T) / V → (2.34 moles.  0.082L.atm/mol.K . 273 K) / 11.08L = 4.73atm

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