a)Would you expect the empirical formula you determine for magnesium oxide to be the same as the one determined by another student?
b) Would you expectan empirical formulato be the same even though different masses of Mg were used? Briefly explain.
c) If different masses of mg are used,account for any difference in the empirical formulas.
a) It is likely that the empirical formula determined for magnesium oxide would be the same as the one determined by another student if the experiment was conducted correctly and the same procedure was followed. The empirical formula represents the simplest whole number ratio of atoms in a compound, so as long as the measurements and calculations are accurate, the empirical formula should be consistent across different experiments.
b) Yes, even if different masses of magnesium (Mg) were used, we would still expect the empirical formula to be the same. This is because the empirical formula is determined by the ratio of the number of atoms of each element in the compound, not the actual masses used. As long as the ratio remains the same, the empirical formula will not change.
c) If different masses of magnesium are used, it may impact the quantities of the elements present in the compound, but it should not affect the empirical formula. Regardless of the mass used, the empirical formula is determined by the ratio of the number of atoms of each element. The masses used will only affect the absolute quantities of each element, but the ratio will remain constant.
a) No, it is not necessary that the empirical formula determined for magnesium oxide by another student will be the same. The empirical formula is determined based on the ratio of the number of atoms of each element in a compound, and it depends on accurate measurement and experimental procedure. If there are any errors or variations in the experimental procedure or measurement, it can lead to different empirical formulas.
b) Yes, even though different masses of magnesium (Mg) were used, we would still expect the empirical formula to be the same. This is because the empirical formula is based on the ratio of the number of atoms of each element in a compound, rather than the actual masses used. As long as the ratio remains the same, the empirical formula will remain the same. For example, if the ratio of Mg to O is 1:1, it means for every 1 atom of Mg, there is 1 atom of O. It doesn't matter if 10 grams of Mg or 20 grams of Mg were used, as long as the ratio remains 1:1, the empirical formula will be the same.
c) If different masses of Mg are used, it can affect the stoichiometric ratio between magnesium and oxygen in the compound. The empirical formula is based on the simplest whole-number ratio of atoms in a compound. So, if different masses of Mg are used, the ratio between Mg and O may change, resulting in a different empirical formula.
For example, if the ratio of Mg to O is 1:1, and we use 10 grams of Mg, it means we have 10 moles of Mg. However, if we use 20 grams of Mg, it means we have 20 moles of Mg. This change in the number of moles can lead to a different ratio between Mg and O, and thus a different empirical formula.
To account for any difference in the empirical formulas when different masses of Mg are used, it is essential to convert the masses of Mg into moles using the molar mass. Then, compare the ratios of Mg to O to determine the empirical formula.