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Ch.10 - Gases
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.10 - Gases문제 108
10장, 문제 108

An 8.40-g sample of argon and an unknown mass of H2 are mixed in a flask at room temperature. The partial pressure of the argon is 44.0 kPa, and that of the hydrogen is 57.33 kPa. What is the mass of the hydrogen?

검증된 단계별 안내
1
Identify the known values: mass of argon (8.40 g), partial pressure of argon (44.0 kPa), and partial pressure of hydrogen (57.33 kPa).
Use the ideal gas law in the form of \( PV = nRT \) to find the number of moles of argon. Assume the volume and temperature are constant for both gases.
Calculate the number of moles of argon using its molar mass (39.95 g/mol) and the given mass.
Use the ratio of partial pressures to find the number of moles of hydrogen, since \( \frac{P_{\text{H}_2}}{P_{\text{Ar}}} = \frac{n_{\text{H}_2}}{n_{\text{Ar}}} \).
Calculate the mass of hydrogen using the number of moles of hydrogen and its molar mass (2.02 g/mol).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Dalton's Law of Partial Pressures

Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle allows us to analyze the behavior of gases in a mixture, as each gas contributes to the total pressure independently of the others.
추천 영상:
가이드 코스
00:27
Dalton's Law and Partial Pressure

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the properties of gases under various conditions and can be used to find the number of moles of hydrogen in this scenario, given its partial pressure.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula

Molar Mass and Mass Calculations

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. To find the mass of hydrogen in the mixture, we can first determine the number of moles using the Ideal Gas Law and then convert this to mass using the molar mass of hydrogen (approximately 2.02 g/mol).
추천 영상:
가이드 코스
03:12
Molar Mass Calculation Example
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교과서 질문

Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (a) If the total pressure of the gases is 99.8 kPa, calculate the partial pressure of each component of the mixture.

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교과서 질문

Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (b) If the volume of the exhaled gas is 455 mL and its temperature is 37 °C, calculate the number of moles of CO2 exhaled.

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교과서 질문
An ideal gas at a pressure of 152 kPa is contained in a bulb of unknown volume. A stopcock is used to connect this bulb with a previously evacuated bulb that has a volume of 0.800 L as shown here. When the stopcock is opened, the gas expands into the empty bulb. If the temperature is held constant during this process and the final pressure is 92.66 kPa, what is the volume of the bulb that was originally filled with gas?

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교과서 질문

Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (c) How many grams of glucose (C6H12O6) would need to be metabolized to produce this quantity of CO2? (The chemical reaction is the same as that for combustion of C6H12O6. See Section 3.2 and Problem 10.57.)

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교과서 질문

The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (a) Determine a precise molar mass for the gas. [Hint: Graph d>P versus P.]

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교과서 질문

The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (b) Why is d>P not a constant as a function of pressure?

619
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