Examination reveals that 180.2 g/mol of glucose contains 72.1 grams of carbon, 96 g/mol of oxygen and the remainder is hydrogen.
1 answer:
Mass of Hydrogen = 3.7 g
<h3>Further explanation </h3>The empirical formula is the smallest comparison of atoms of compound forming elements.
A molecular formula is a formula that shows the number of atomic elements that make up a compound.
(empirical formula) n = molecular formula
180.2 g/mol of glucose-C₆H₁₂O₆ contains 72.1 grams of carbon, 96 g/mol of oxygen and the remainder is hydrogen
Remainder Hydrogen :
% mass of Hidrogen in Gllucose :
So mass of Hydrogen in 55.5 g Glucose :
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Answer:
The presence of the contaminant increases the total mass.
And on continuous heating to remove the volatile impurities, the hydrated salt gets overheated and the anhydrous salt gets thermally decomposed thereby producing a gas.
The heating leads to the formation or release of a gas which leads to loss of a higher percentage of mass from the compound making the mass percent of water in the hydrated salt too high and the mass of the anhydrous salt remaining in the crucible too low.
Hydrated Salt ⇒ Anhydrous salt + Water hydration