Mercury can be obtained by reacting mercury(II) sulfide with calcium oxide. How many grams of Mercury metal are produced when 2.11 g of calcium oxide reacts with excess mercury(II) sulfide? 4HgS+4CaO=4Hf+3CaS+CaSO4

a. 10.1 g

b. 1.80 g

c. 13.4 g

d. 7.56 g

Option D. 7.56 g of Hg.

Explanation:

The balanced equation for the reaction is given below:

4HgS + 4CaO —> 4Hg + 3CaS + CaSO₄

Next, we shall determine the mass of CaO that reacted and the mass of Hg produced from the balanced equation. This is can be obtained as follow:

Molar mass of CaO = 40 + 16

= 56 g/mol

Mass of CaO from the balanced equation = 4 × 56 = 224 g

Molar mass of Hg = 200.59 g/mol

Mass of Hg from the balanced equation = 4 × 200.59 = 802.36 g

SUMMARY

From the balanced equation above,

224 g of CaO reacted to produce 802.36 g of Hg.

Finally, we shall determine the mass of Hg produced by the reaction of 2.11 g of CaO. This can be obtained as follow:

From the balanced equation above,

224 g of CaO reacted to produce 802.36 g of Hg.

Therefore, 2.11 g of CaO will react to produce = (2.11 × 802.36)/224 = 7.56 g of Hg.

Thus, 7.56 g of Hg were obtained from the reaction.

the answer would be c

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