Ch.6 - Gases

Tro - Chemistry: A Molecular Approach 6th Edition

Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217당신이 사용하는 게 아니라요?교과서 변경

Tro 6th Edition

Ch.6 - Gases

문제 99

6장, 문제 99

Which postulate of the kinetic molecular theory breaks down under conditions of high pressure? Explain.

검증된 단계별 안내

Identify the postulates of the kinetic molecular theory, which include: 1) Gas particles are in constant, random motion. 2) The volume of the gas particles is negligible compared to the volume of the container. 3) Gas particles exert no forces on each other; they neither attract nor repel each other. 4) Collisions between gas particles and with the walls of the container are perfectly elastic. 5) The average kinetic energy of gas particles is proportional to the temperature in Kelvin.

Recognize that under high pressure, the volume of the gas particles becomes significant compared to the volume of the container.

Understand that at high pressure, gas particles are much closer together, which means the assumption that gas particles exert no forces on each other (postulate 3) breaks down.

Explain that under these conditions, intermolecular forces become significant, leading to deviations from ideal gas behavior.

Conclude that the postulate stating that gas particles exert no forces on each other is the one that breaks down under high pressure conditions.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

45s

도움이 되었나요?

주요 개념

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

Kinetic Molecular Theory

The Kinetic Molecular Theory (KMT) describes the behavior of gases in terms of particles in constant motion. It posits that gas particles are small, have negligible volume, and experience elastic collisions. This theory helps explain gas properties such as pressure, temperature, and volume, providing a framework for understanding gas behavior under various conditions.

Ideal Gas Behavior

Ideal gas behavior refers to the assumption that gas particles do not interact with each other and occupy no volume. This behavior is described by the Ideal Gas Law (PV=nRT), which holds true under low pressure and high temperature. However, deviations from ideal behavior occur at high pressures, where particle volume and intermolecular forces become significant.

High Pressure Effects

Under high pressure, the assumptions of the Kinetic Molecular Theory begin to break down because gas particles are forced closer together, leading to significant intermolecular forces and a noticeable volume of the particles themselves. This results in deviations from the Ideal Gas Law, as real gases do not behave ideally under such conditions, affecting their pressure, volume, and temperature relationships.

관련 실천

교과서 질문

A sample of CO2 effuses from a container in 55 seconds. How long will it take the same amount of gaseous Xe to effuse from the same container under identical conditions?

views

교과서 질문

Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of neon at a pressure of 500.0 atm and a temperature of 355.0 K. Explain why the two values are different. (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V.)

3749

views

교과서 질문

The graph shows the distribution of molecular velocities for the same molecule at two different temperatures (T₁ and T₂). Which temperature is greater? Explain.

602

views

교과서 질문

Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000 mol of Cl₂ in a volume of 5.000 L at a temperature of 273.0 K. Explain why the two values are different.

Modern pennies are composed of zinc coated with copper. A student determines the mass of a penny to be 2.482 g and then makes several scratches in the copper coating (to expose the underlying zinc). The student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the HCl (the copper remains undissolved): Zn(s) + 2 HCl(aq)¡ H2( g) + ZnCl2(aq) The student collects the hydrogen produced over water at 25 °C. The collected gas occupies a volume of 0.899 L at a total pressure of 791 mmHg. Calculate the percent zinc (by mass) in the penny. (Assume that all the Zn in the penny dissolves.)

The graph shows the distribution of molecular velocities for two different molecules (A and B) at the same temperature. Which molecule has the higher molar mass? Which molecule has the higher rate of effusion?

1584

views

rank