3. A sample of pure iron was covered with an excess of powdered elemental sulfur

Question

3. A sample of pure iron was covered with an excess of powdered elemental sulfur. The mixture was heated to a temperature where a reaction occurred and the excess sulfur was volatilized. The following data were collected. Complete the table. Record the calculated values with the correct number of significant figures a. Mass of crucible and lid (3) 19.746 20422 21.004 b. Mass of crucible, lid and iron sample (g) c. Final Mass of crucible, lid, and compound (g) e. Mass of Iron (g) f. Moles of Iron (mol) g. Mass of compound (9) · · h. Mass of Sulfur in compound (g) i. Moles of Sulfur in compound (mol) j. Mole ratio of Iron to Sulfur k. Empirical formula of compound I, % by mass iron in compound m. % by mass sulfur in compound n. Write a balanced equation for the reaction that occurred.

Explanation / Answer

e. mass of iron = 6.76 x 10-1 g

f.moles of iron = mass / molar mass = .676 / 55.84 = 0.012 mole

g. mass of compound = 1,258 g

h. mass of sulphur = mass of compound - mass of iron = 1.258-.676 = 5.82 x 10-1g

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