Solving 3 Gas Mixture: Assumptions & PV=mRT

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The discussion focuses on the behavior of a gas mixture in a rigid container, specifically analyzing the pressures of three gases: A, B, and C, under the ideal gas law PV=mRT. Key assumptions include the ideal gas behavior of the gases and the constancy of volume during the pressure measurements. The pressure readings P[T], P[A], P[B], and P[C] are critical for understanding the relationship between the gases in the mixture. The unit for "amount of gas" is typically measured in moles, allowing for direct comparison across different gases.

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1. A rigid container is filled with a mixture of three gases: A, B and C. the pressure gauge reads P[T]. The container is evacuated and fill with an amount of gas A equal to that in the original mixture. The gauge now reads P[A]. This process is repeated for gases B and C with the pressure gauge reading P and P[C]? What assumptions are made?



2. PV=mRT



3. The gases are related by the volume because they might have different pressures, temperatures and mass.
 
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I don't see any assumptions made (apart from "the container is filled with gas 4 times"), as there is no analysis described.
I guess an analysis will assume that volume is constant, and it might be a reasonable assumption that all gases are ideal.

What is the unit for "amount of gas" to compare different gases?
 

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