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

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To calculate the mass of each gas component in a heated mixture of oxygen, carbon dioxide, and nitrogen, the ideal gas law (PV=NRT) can be applied, but the initial data is insufficient. The mixture's composition is given as 0.1 oxygen, 0.2 carbon dioxide, and 0.7 nitrogen, but it's unclear whether these values represent mass or molar ratios. The molar mass of the mixture can be calculated using the formula 0.7(28) + 0.2(44) + 0.1(32), which helps in determining the mass once the number of moles is known. However, without clarification on the ratios, the calculation remains ambiguous. Accurate mass determination requires more specific information regarding the ratios of the components.
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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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