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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An "ideal" fuel/air mixture in which both the fuel and the oxygen in the air are completely consumed is called the "stoichiometric" mixture. The stoichiometric mixture is usually specified as the ratio of the mass of air to the mass of a particular fuel. For example, if a fuel (for example, natural gas, CH4) required 17.2 kg of air to precisely burn 1 kg of the fuel (that is, all the fuel burned and there was no oxygen left in the air afterwards) then the stoichiometric ratio for that fuel would be 17.2: 1. Calculate the partial pressures of the natural gas and oxygen in the mixture based on the stoichiometric ratio given above at 293.15 K. The volume of the internal combustion engine is considered to be 2.500 L. The mass of the fuel is 160.0 g. Mass fraction of oxygen in air is 23.1%. Molar mass of natural gas is 16.043 g/mol. atm natural gas = Poxygen atm

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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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An "ideal" fuel/air mixture in which both the fuel and the oxygen in the air are completely consumed is called the "stoichiometric" mixture. The stoichiometric mixture is usually specified as the ratio of the mass of air to the mass of a particular fuel. For example, if a fuel (for example, natural gas, CH4) required 17.2 kg of air to precisely burn 1 kg of the fuel (that is, all the fuel burned and there was no oxygen left in the air afterwards) then the stoichiometric ratio for that fuel would be 17.2: 1. Calculate the partial pressures of the natural gas and oxygen in the mixture based on the stoichiometric ratio given above at 293.15 K. The volume of the internal combustion engine is considered to be 2.500 L. The mass of the fuel is 160.0 g. Mass fraction of oxygen in air is 23.1%. Molar mass of natural gas is 16.043 g/mol. atm natural gas = Poxygen atm

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