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Mercury (Hg) is typically obtained from the ore Cinnabar, mercury (II) sulfide (HgS), according to the following balanced chemical reaction:  HgS(s) + O2(g) --> Hg(l) + SO2(g) Suppose the reaction was carried out to completion and 21.55 mL Hg(l) were obtained without any losses (in other words, the percent yield of the reaction was 100%). Note, the density of liquid mercury is 13.5 g/mL. a) In the space below, write the appropriate mole-mole ratio needed to determine the amount of SO2(g) from the given information. Include the correct numbers, units, and formulas. b) What was the total mass, in grams, of SO2(g) that was produced from the reaction?

Mercury (Hg) is typically obtained from the ore Cinnabar, mercury (II) sulfide (HgS), according to the following balanced chemical reaction:  HgS(s) + O2(g) --> Hg(l) + SO2(g) Suppose the reaction was carried out to completion and 21.55 mL Hg(l) were obtained without any losses (in other words, the percent yield of the reaction was 100%). Note, the density of liquid mercury is 13.5 g/mL. a) In the space below, write the appropriate mole-mole ratio needed to determine the amount of SO2(g) from the given information. Include the correct numbers, units, and formulas. b) What was the total mass, in grams, of SO2(g) that was produced from the reaction?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section3.6: The Mole And Chemical Reactions
Problem 3.17E
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Mercury (Hg) is typically obtained from the ore Cinnabar, mercury (II) sulfide (HgS),
according to the following balanced chemical reaction: 
HgS(s) + O2(g) --> Hg(l) + SO2(g)

Suppose the reaction was carried out to completion and 21.55 mL Hg(l) were obtained without
any losses (in other words, the percent yield of the reaction was 100%). Note, the density of
liquid mercury is 13.5 g/mL.

a) In the space below, write the appropriate mole-mole ratio needed to determine the amount
of SO2(g) from the given information. Include the correct numbers, units, and formulas.

b) What was the total mass, in grams, of SO2(g) that was produced from the reaction?

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