Kuya,
Percent purity is bugging me...
Problems like:
A 0.7500 gram sample containing Aluminum metal and sand was analyzed. If 0.548 Liters of H2(g) was collected at 20.0°C, what was the mass % of Al(s) in the sample? The vapor pressure of water is 17.54 torr at 20.0°C and the atmospheric pressure was 755.3 torr during the experiment.
I identified units of Mass, Volume, Pressure, and Temperature, which corresponds to the ideal gas law, PV=nRT; R being equivalent to the constant, (0.082057L•atm/K•mol)
After converting to the standard units, I am given:
*0.2800 moles of Aluminum metal
0.548 Liters of H2(g) collected at 293.15K
The vapor pressure of water: 0.2300 atm at 293.15K
and finally, the atmospheric pressure: 0.9940 atm
*I am a little stuck here, because one, it seems like my conversion from grams to moles seems invalid because it is a mixture containing both Aluminum metal and Sand as opposed to just Aluminum alone.
So our main goal is to find the percent yield in correlation to purity. So you already defined the the Ideal Gas Law, which is (PV=nRT):
In this case, P is the absolute gas presure, okay.
In this case, the given V is volume of given gas.
In this case n correlates for gas molecules.
In this case R is the universal gas constant.
In this case T is the absolute temp.
You already provided the universal gas constant as being: (0.082057L•atm/K•mol)
And you already provided the data; so let us apply it.
Theoretically IGL: PV=nRT
Therefore, calculate your data.
What I would do is to utilize boltzman's constant (k) as substitute in order to make this simpler.
When you have your data, find the % purity by the equation:
actual mass obtained/ calculated mass x 100%
Then you should have your answer.
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