Question

Dalton's Law of Partial Pressures In a mixture of gases the total pressure, PT, is the sum of the pressures of the individual gases, P1, etc. PT = P1 + P2 + P3+... Since each gas behaves independently, the ideal gas law can be used to calculate the pressure of that gas. In other words, each gas exerts the same pressure as it would exert if it was in the container alone. The pressure of a gas in a mixture is represented by: P1 = (n1RT) / V 6. A 2.00 L container holds 4.00 moles of O2 and 2.70 moles of He at 293 K. What is the partial pressure of O2? Of He? What is the total pressure? 7. Consider the three flasks in the figure below. Assume that the connecting tubes have no volume and the temperature is held constant (Hint: you won't need the ideal gas law; think about pressure versus volume). He 1.0 L 200 torr Ne 1.0 L 410 torr Ar 2.0 L 250 torr a) Calculate the partial pressure of each gas when all stopcocks are open. b) Calculate the total pressure when all stopcocks are open.

          Dalton's Law of Partial Pressures
In a mixture of gases the total pressure, PT, is the sum of the pressures of the individual gases, P1, etc.
PT = P1 + P2 + P3+...
Since each gas behaves independently, the ideal gas law can be used to calculate the pressure of that gas. In other words, each gas exerts the same pressure as it would exert if it was in the container alone. The pressure of a gas in a mixture is represented by:
P1 = (n1RT) / V
6. A 2.00 L container holds 4.00 moles of O2 and 2.70 moles of He at 293 K. What is the partial pressure of O2? Of He? What is the total pressure?
7. Consider the three flasks in the figure below. Assume that the connecting tubes have no volume and the temperature is held constant (Hint: you won't need the ideal gas law; think about pressure versus volume).
He 1.0 L 200 torr
Ne 1.0 L 410 torr
Ar 2.0 L 250 torr
a) Calculate the partial pressure of each gas when all stopcocks are open.
b) Calculate the total pressure when all stopcocks are open.

Dalton's Law of Partial Pressures
In a mixture of gases the total pressure, PT, is the sum of the pressures of the individual gases, P1, etc.
PT = P1 + P2 + P3+...
Since each gas behaves independently, the ideal gas law can be used to calculate the pressure of that gas. In other words, each gas exerts the same pressure as it would exert if it was in the container alone. The pressure of a gas in a mixture is represented by:
P1 = (n1RT) / V
6. A 2.00 L container holds 4.00 moles of O2 and 2.70 moles of He at 293 K. What is the partial pressure of O2? Of He? What is the total pressure?
7. Consider the three flasks in the figure below. Assume that the connecting tubes have no volume and the temperature is held constant (Hint: you won't need the ideal gas law; think about pressure versus volume).
He 1.0 L 200 torr
Ne 1.0 L 410 torr
Ar 2.0 L 250 torr
a) Calculate the partial pressure of each gas when all stopcocks are open.
b) Calculate the total pressure when all stopcocks are open.

Added by James H.

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