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For each reaction, calculate how many moles of the product form when 0.112 mol of the
Chapter 0, Problem 22(choose chapter or problem)
For each reaction, calculate how many moles of the product form when \(0.112 \mathrm{~mol}\) of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) \(2 \ \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{CaO}(s)\)
(b) \(4 \ \mathrm{Fe}(s)+3 \ \mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\)
(c) \(4 \mathrm{~K}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~K}_{2} \mathrm{O}(s)\)
(d) \(4 \ \mathrm{Al}(s)+3 \ \mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{Al}_{2} \mathrm{O}_{3}(s)\)
Questions & Answers
QUESTION:
For each reaction, calculate how many moles of the product form when \(0.112 \mathrm{~mol}\) of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) \(2 \ \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{CaO}(s)\)
(b) \(4 \ \mathrm{Fe}(s)+3 \ \mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\)
(c) \(4 \mathrm{~K}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~K}_{2} \mathrm{O}(s)\)
(d) \(4 \ \mathrm{Al}(s)+3 \ \mathrm{O}_{2}(g) \longrightarrow 2 \ \mathrm{Al}_{2} \mathrm{O}_{3}(s)\)
ANSWER:Step 1 of 5
From the given data, the moles of reactant is 0.112 mol.
The moles of product formed are to be determined.