2. When the molecular weight of carbon dioxide in lab, it is likely that some wa

Question

2. When the molecular weight of carbon dioxide in lab, it is likely that some water vapor was present in the sample of gas trapped in the inverted beaker This is true whenever we collect a gas over water. Lets also assume that the pressure of the atmosphere was less than 1.0 atm on the day of the experiment. We now have two reasons to believe that the actual pressure of carbon dioxide gas was not 1.0 atm, but might have been as low as 0.90 atm. How would this impact your value for the molecular weight of carbon dioxide? 2. When the molecular weight of carbon dioxide in lab, it is likely that some water vapor was present in the sample of gas trapped in the inverted beaker This is true whenever we collect a gas over water. Lets also assume that the pressure of the atmosphere was less than 1.0 atm on the day of the experiment. We now have two reasons to believe that the actual pressure of carbon dioxide gas was not 1.0 atm, but might have been as low as 0.90 atm. How would this impact your value for the molecular weight of carbon dioxide?

Explanation / Answer

This can be solved by using following formula,

molar mass= R*T*density/P,

where R= gas constant, T= temp. in K, P= presure in atm,

by putting the values to the equation,

Molar mass= 0.0821*373 K*1/0.90 (Temp. 273+ 100 373 K),

Molar mass =30.6233/0.90,

molar mass= 34.02 g/mol

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