This is to be explained why the measured properties of a mixture of gases depend only on the total number of moles of particles but not on the identity of individual gas particles. Concept Introduction: In an ideal gas, molecules are assumed to occupy negligible volume. This means the interaction between the molecule of gas is negligible in case of ideal gases. Due to this there is no difference between substance as per the molecules of gas as far as behavior is concerned for the bulk amount. All the gas molecules independently behave and the overall amount of gas present in the system determined the overall propertied of the sample. According to the Dalton’s law of partial pressures, if a mixture of gasses is present in a container, the total pressure exerted by gas molecules will be sum of the partial pressures of all the gases present in the container. Here, the partial pressure of a gas is defined as pressure exerted by a gas when it is considered alone in the container.

Question

The temperature on a sample of pure X held at 1.25 atm and -54. °C is increased until the sample boils. The temperature is then held constant and the pressure is decreased by 0.42 atm. On the phase diagram below draw a path that shows this set of changes. pressure (atm) 2 0 0 200 400 temperature (K) X

Answer 1

Question

Chapter 13, Problem 65QAP

Interpretation Introduction

Interpretation:

This is to be explained why the measured properties of a mixture of gases depend only on the total number of moles of particles but not on the identity of individual gas particles.

Concept Introduction:

In an ideal gas, molecules are assumed to occupy negligible volume. This means the interaction between the molecule of gas is negligible in case of ideal gases.

Due to this there is no difference between substance as per the molecules of gas as far as behavior is concerned for the bulk amount. All the gas molecules independently behave and the overall amount of gas present in the system determined the overall propertied of the sample.

According to the Dalton’s law of partial pressures, if a mixture of gasses is present in a container, the total pressure exerted by gas molecules will be sum of the partial pressures of all the gases present in the container. Here, the partial pressure of a gas is defined as pressure exerted by a gas when it is considered alone in the container.

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