객관식
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?
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11 Gases
Dalton's Law: Partial Pressure (Simplified)
객관식
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?
A
220 mmHg
B
242 mmHg
C
588 mmHg
D
183 mmHg
검증된 단계별 안내1
Step 1: Understand that the partial pressure of a gas in a mixture can be determined using Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas.
Step 2: Calculate the mass of each gas in the mixture. Assume a sample size, for example, 100 grams, to simplify calculations. This means the sample contains 72.8 grams of chlorine and 27.2 grams of neon.
Step 3: Determine the number of moles of each gas using their molar masses. The molar mass of chlorine (Cl₂) is approximately 70.9 g/mol, and the molar mass of neon (Ne) is approximately 20.18 g/mol. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
Step 4: Calculate the mole fraction of neon in the mixture. The mole fraction is the ratio of the moles of neon to the total moles of gases in the mixture. Use the formula: \( \text{mole fraction of Ne} = \frac{\text{moles of Ne}}{\text{moles of Cl₂} + \text{moles of Ne}} \).
Step 5: Apply Dalton's Law to find the partial pressure of neon. Multiply the mole fraction of neon by the total pressure of the gas mixture: \( \text{partial pressure of Ne} = \text{mole fraction of Ne} \times \text{total pressure} \).
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