How Do You Calculate the Mass of Each Gas Component in a Heated Mixture?

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SUMMARY

The discussion focuses on calculating the mass of each gas component in a heated mixture consisting of 0.1 oxygen, 0.2 carbon dioxide, and 0.7 nitrogen at initial conditions of 300 K and 100 kPa, later heated to 500 K and 300 kPa. Participants suggest using the ideal gas law (PV=NRT) to find the number of moles, but note the ambiguity in the ratios provided, as it is unclear whether they represent mass or molar ratios. The molar mass of the mixture is calculated as 28 g/mol for nitrogen, 44 g/mol for carbon dioxide, and 32 g/mol for oxygen, leading to a total molar mass of 32.4 g/mol for the mixture.

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1. A mixture at T=300 K and P=100 kPa is made up of .1 oxygen, .2 carbon dioxide, and .7 Nitrogen. It is then heated to 300 kPa and 500 K. Find the mass of each component


I originally thought using PV=NRT, ideal gas but there doesn't seem to be enough givens. Can you also find the molar mass of the mixture by doing:

.7(28)+.2(44)+.1(32), so then you can find the mass of the component when you find the number of moles N but I am having problems doing that
 
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Yes, the question is incomplete. In addition, it's ambiguous, as it does not state whether .1, .2 and .7 are mass or molar (ie, volume) ratios (assuming they are ratios).
 

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