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In certain lung ailments such as emphysema, there is adecrease in the ability of oxygen to diffuse into the blood.a. How would the partial pressure of oxygen in the blood change?
8. Gases, Liquids and Solids
Dalton's Law: Partial Pressure (Simplified)
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple 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?
A
220 mmHg
B
242 mmHg
C
588 mmHg
D
183 mmHg
Verified step by step guidance1
First, 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 partial pressure of a gas is equal to the mole fraction of the gas multiplied by the total pressure of the mixture.
Calculate the mole fraction of neon in the mixture. To do this, assume a sample size, for example, 100 grams of the gas mixture. This means you have 72.8 grams of chlorine and 27.2 grams of neon.
Convert the mass of each gas to moles 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.
Calculate the mole fraction of neon by dividing the moles of neon by the total moles of the gas mixture.
Finally, apply Dalton's Law: multiply the mole fraction of neon by the total pressure (809 mmHg) to find the partial pressure of neon.
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