In my experiment I heated some oxide of tin, in order to figure out its empirical formula.
How would the empirical formula be affected if the oxide was not heated to dryness?
Also
If some oxide splattered out of the container, how would this affect the calculated ration of the number of moles of oxygen to the number of moles of tin?
Thank You
You would be recording a mass for Sn highter than you should, as it contains H2O
If the oxide of tin is not heated to dryness, it can affect the determination of its empirical formula. Heating to dryness is typically done to ensure that all the moisture and impurities present in the sample are driven off, resulting in a more accurate measurement of the pure substance.
If the oxide is not heated to dryness, it might still contain some impurities or moisture, which can change the composition of the sample. These impurities or moisture will contribute to the overall mass of the compound, and as a result, the calculated empirical formula may not accurately represent the true ratio of atoms in the compound.
Therefore, it is important to heat the oxide of tin to dryness and remove any impurities or moisture before determining its empirical formula.
Regarding the splattering of oxide out of the container, it would also affect the calculated ratio of the number of moles of oxygen to the number of moles of tin.
When the oxide splatters out of the container, it means some of the sample is lost. This loss of material will lead to an underestimation of the total mass of the compound. Consequently, the calculated ratio of moles of oxygen to moles of tin will be lower than the actual ratio.
To obtain accurate results, it is crucial to ensure that all the oxide of tin remains in the container during the experiment. Any loss or splattering of the sample will affect the calculated empirical formula and ratio of moles.