How Is the Molar Mass of Gas X Calculated?

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To calculate the molar mass of gas X, the mass of the gas is found by subtracting the mass of the empty flask from the mass of the filled flask, resulting in 0.3334g. The volume of gas X is converted from 250cm³ to 0.25 dm³. The initial calculation of molar mass as 1.3336g/dm³ is incorrect; the correct approach involves using conditions at room temperature and pressure (RTP). Under these conditions, the volume of one mole of gas is approximately 24.2 L, leading to the calculation of moles as 0.01033 mol. The final molar mass is then calculated as 34g/mol, indicating a mistake in the initial method.
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the mass of a 250cm3 round bottomed flask is filled with gas X is determined to be 16.2850g. the mass of the empty flask and stopper is 15.9516g. what is the molar mass of gas X?

am i right to do it this way:

mass of gas X alone = 16.2850 - 15.9516 = 0.3334g
volume of gas X = 250/1000 = 0.25 dm3

molar mass of gas X = 0.3334/0.25 = 1.3336g/dm3

however, the answer is 32g, where did i make a mistake?

thank you
 
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what conditions are you working under?? STP?

molar mass= g/mol
not g/L

If its at room temp then you have:
295K
1 atm
24.2 L/mol

.250L/(24.2L/mol)= .01033mol

.3334g/.01033mol= 34g/mol
 
Last edited:
working under rtp

thank you
 

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