Skip to main content
Ch.10 - Gases
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.10 - Gases문제 105
10장, 문제 105

An ideal gas at a pressure of 1.50 atm 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 695 torr, what is the volume of the bulb that was originally filled with gas?

검증된 단계별 안내
1
Convert the initial pressure from atm to torr using the conversion factor: 1 atm = 760 torr.
Apply the ideal gas law concept, which states that for a constant temperature and amount of gas, the initial and final states can be related by Boyle's Law: \( P_1V_1 = P_2V_2 \).
Identify the initial conditions: \( P_1 \) is the initial pressure in torr, and \( V_1 \) is the unknown volume of the original bulb.
Identify the final conditions: \( P_2 \) is the final pressure (695 torr), and \( V_2 \) is the total volume after expansion, which is the sum of the unknown volume and 0.800 L.
Rearrange the equation \( P_1V_1 = P_2V_2 \) to solve for \( V_1 \), the volume of the bulb that was originally filled with gas.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
3m

주요 개념

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

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of an ideal gas through the equation PV = nRT. In this scenario, understanding how pressure and volume interact at constant temperature is crucial for solving the problem. The law helps predict how gas will behave when it expands or contracts.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula

Boyle's Law

Boyle's Law states that for a given mass of gas at constant temperature, the pressure of the gas is inversely proportional to its volume (P1V1 = P2V2). This principle is essential for analyzing the gas expansion in the question, as it allows us to relate the initial and final states of the gas when the stopcock is opened.
추천 영상:
가이드 코스
03:13
Boyle's Law

Pressure Conversion

In this problem, pressure is given in different units (atm and torr), so understanding how to convert between these units is vital. The conversion factor is 1 atm = 760 torr. Accurately converting pressures ensures that calculations involving Boyle's Law and the Ideal Gas Law are correct and consistent.
추천 영상:
가이드 코스
02:20
Pressure Conversion Example
관련 실천
교과서 질문

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (d) Which one has the highest total molecular volume relative to the space occupied by the gas?

626
views
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 0.985 atm, calculate the partial pressure of each component of the mixture.

1
views
교과서 질문

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (a) Which gas is most likely to depart from the assumption of the kinetic-molecular theory that says there are no attractive or repulsive forces between molecules?

1083
views
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.)

518
views
교과서 질문

You have a sample of gas at −33°C. You wish to increase the rms speed by a factor of 2. To what temperature should the gas be heated?

2
views
교과서 질문

A 1.42-g sample of helium and an unknown mass of O2 are mixed in a flask at room temperature. The partial pressure of the helium is 42.5 torr, and that of the oxygen is 158 torr. What is the mass of the oxygen?

1
views