Concept explainers
Lead(ll) oxide is obtained by roasting galena, lead(ll) sulfide, in air. The unbalanced equation is:
a. Balance the equation, and determine the theoretical yield of
b. What is the percent yield if 170.0 g of
a)
Interpretation : The balanced equation of chemical reaction is to be written and theoretical yield needs to be calculated.
Concept introduction : Lead oxide is obtained by roasting galena. Galena is an ore of Lead.
Roasting: It is a process to heat ore (sulphite, carbonate, sulphide) in presence of oxygen to convert it into oxide of metal.
Answer to Problem 91A
Theoretical yield is 187.47 g of PbO
Explanation of Solution
Step 1: Write balance chemical equation:
Step 2: convert mass of reactant to moles
Step 3: Convert moles of reactant to moles of product using mole ratio
2 moles of PbS produce = 2 moles of PbO
1 moles of PbS produce = 1 moles of PbO
0.84 moles of PbS produce = 0.84 moles of PbO
Step 4: Convert moles of product to mass (theoretical yield)
b)
Interpretation:
If 170g of PbO was produce, the percent yield needs to be determined.
Concept introduction:
The percent yield can be calculated as follows:
Answer to Problem 91A
Percent yield = 90.68%
Explanation of Solution
Actual yield = 170 g (given)
Chapter 11 Solutions
Glencoe Chemistry: Matter and Change, Student Edition
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