1. For the following reaction, 6.90 grams of magnesium nitride are mixed with ex

Question

1. For the following reaction, 6.90 grams of magnesium nitride are mixed with excess water. The reaction yields 11.3 grams of magnesium hydroxide.

Mg3N2(s) + 6H2O (l) ---> 3Mg(OH)2 (aq) + 2NH3(aq)

2. For the following reaction, 3.67 grams of chlorine gas are mixed with excess carbon disulfide. The reaction yields 1.46 grams of carbon tetrachloride.

CS2(s) + 4Cl2 (g) ---> CCl4 (l) + 2SCl2 (s)

Explanation / Answer

Question 1

Balanced equation:
Mg3N2(s) + 6 H2O(l) =====> 3 Mg(OH)2(aq) + 2 NH3(aq)
Reaction type: double replacement
6.90 grams of magnesium nitride = 6.9 / 100.92 = 0.06836 Moles

Moles of of magnesium hydroxide produced = 0.20509 Moles

mass of magnesium hydroxide produced = 0.20509 x 58.31 =  11.96 gm

percent yield of magnesium hydroxide =  11.3 x 100 / 11.96 = 94.48 %

Quesiton 2

Balanced equation:
CS2(s) + 4 Cl2(g) =====> CCl4(l) + 2 SCl2(s)
Reaction type: double replacement

3.67 grams of chlorine gas = 3.67 / 70.9 = 0.0517 Moles

Moles of carbon tetrachloride produced =  0.012939 Moles

Mass of carbon tetrachloride produced =  0.012939 Moles 153.82 gm/mol =  1.990 gm

percent yield of carbon tetrachloride produced = 1.46 x 100 / 1.990 = 73.36 %

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.