Pure component volume

The above method is commonly used for gases and infrequently for liquid mixtures. At atmospheric conditions when ideal gas behavior is realized, the total volume of the mixture equals the sum of the pure-component volumes ( V ). That is, V = V and... 

Amagat S Law. The total volume of a gaseous mixture equals the sum of the pure-component volumes. By definition, the pure-component volume of a component gas in a mixture is the hypothetical volume that the component would occupy at the same temperature and total pressure of the mixture. By Amagat s law,... 

If each component gas as well as the mixture obeys the ideal gas law, it follows that the pure-component volume of component i is... 

Suppose A moles of substance A. b moles of B, c moles of C, and so on, are contained in a volume R at a temperature T and total pressure P. The partial pressure pA and pure-component volume va of A in the mixture are defined as follows ... 

A similar series of calculations can be performed for pure-component volumes ... 

An ideal gas mixture at 10 bar absolute and 200°C in a 100-m tank contains 50 mole% H2 and 50 mole% N2- What is the partial pressure of H2 What is the pure-component volume of H2 What would happen to pH2 tin, if the temperature were raised ... 

A storage tank contains a gaseous mixture comprised of 30% CO2, 5% CO, 5% H2O, 50% N2, and 10% O2, by volume. What is the partial pressure of each component if the total pressiu-e is 2 atm What are their pure-component volumes if the total volume is 10 tf What are their concentrations in ppm (parts per million) ... 

Amagat s law states that the pure component volume, of an ideal gas is given by... 

The volume contribution of chlorine to the total volume,, often referred to as the pure component volume, is... 

The most significant limitation of Equation (1.5) is that aU the pure-component volumes must be at the same temperature and pressure. If the pure components are not all in the same phase at... 

Bit second virial coefficient for pure component /, volume per mole... 

Figure 3.3 Tests of estimating mixture volumes by mole-fraction averaging the pure component volumes. The broken straight lines are the mole-fraction averages of the pure volumes, as computed via (3.4.2). The solid lines are the true mixture volumes taken from [4]. Benzene(l)-carbon tetrachloride(2) liquid mixtures (fop) are at 25°C, 1 atm. The water(l)-ethanol(2) liquid mixtures (bottom) are at 20°C, 1 atm.

The equations given for enthalpy and entropy of ideal-gas mixture were given here without proof. They can be proven using the tools of statistical mechanics, but this is beyond the scope of this book. Nonetheless, we can arrive at these equations by qualitative arguments. Since molecules in the ideal-gas state do not interact, the internal energy of the mixture is the same as the total internal energy of the pure components at same pressure and temperature this means = o. And since the volume of the mixture is the sum of the pure component volumes, we conclude the same for enthalpy, or AHm > = o. 

The total number of moles follows from the given pure component volumes and molar volumes to... 

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