Multiple Choice
A gas mixture contains 72.8% chlorine and 27.2% neon by mass. What is the partial pressure of neon in the mixture if the total pressure is recorded as 809 mmHg?
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11 Gases
Dalton's Law: Partial Pressure (Simplified)
Multiple Choice
The partial pressure of N2 in the air is 593 mmHg at 1 atm. What is the partial pressure of N2 in a bubble of air a scuba diver breathes when he is 66 ft below the surface of the water where the pressure is 3.00 atm?
A
2.34 mmHg
B
1779 mmHg
C
593 mmHg
D
2.28×103 mmHg
E
7.02 mmHg
Verified step by step guidance1
Understand that the partial pressure of a gas is proportional to the total pressure of the mixture. Use Dalton's Law of Partial Pressures, which states that the partial pressure of a gas in a mixture is equal to the mole fraction of the gas times the total pressure.
Identify the initial conditions: the partial pressure of N2 in the air at 1 atm is given as 593 mmHg. This means that the mole fraction of N2 in the air is 593 mmHg / 760 mmHg (since 1 atm = 760 mmHg).
Calculate the mole fraction of N2 using the initial partial pressure and total pressure: \( \text{Mole fraction of } N_2 = \frac{593}{760} \).
Determine the new conditions: the total pressure at 66 ft below the surface is 3.00 atm. Convert this pressure to mmHg: \( 3.00 \text{ atm} \times 760 \text{ mmHg/atm} = 2280 \text{ mmHg} \).
Calculate the new partial pressure of N2 in the bubble using the mole fraction and the new total pressure: \( \text{Partial pressure of } N_2 = \text{Mole fraction of } N_2 \times 2280 \text{ mmHg} \).
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