Solution Found!
Answer: For the reaction shown, calculate how many grams of oxygen form when each
Chapter 8, Problem 31P(choose chapter or problem)
For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts.
\(2 \mathrm{HgO}(s) \rightarrow 2 \mathrm{Hg}(\mathrm{l})+\mathrm{O}_{2}(g)\)
(a) 2.13 g HgO
(b) 6.77 g HgO
(c) 1.55 kg HgO
(d) 3.87 mg HgO
Questions & Answers
QUESTION:
For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts.
\(2 \mathrm{HgO}(s) \rightarrow 2 \mathrm{Hg}(\mathrm{l})+\mathrm{O}_{2}(g)\)
(a) 2.13 g HgO
(b) 6.77 g HgO
(c) 1.55 kg HgO
(d) 3.87 mg HgO
ANSWER:
Step 1 of 4
Given reaction is
\(2\mathrm{\ HgO}(s)\ \rightarrow\ 2\mathrm{\ Hg}(1)+\mathrm{O}_2(g)\)
(a)
Given: \(2.13\ \mathrm{gHgO}\)
We have to find how many grams of \(\mathrm{O}_{2}\) forms
\(\mathrm{M}(\mathrm{HgO})=216.6 \frac{\mathrm{g}}{\mathrm{mol}}\) and \(\mathrm{M}\left(\mathrm{O}_{2}\right)=32 \frac{\mathrm{g}}{\mathrm{mol}}\)
Solution map: \(\mathrm{g\ HgO}\ \rightarrow\mathrm{\ mol\ HgO\ }\rightarrow\mathrm{\ g\ O}_2\ \rightarrow\mathrm{\ mol\ O}_2\)
\(\begin{array}{l}\frac{1\mathrm{mol\ HgO}}{216.6\mathrm{g\ HgO}}\rightarrow\frac{1\mathrm{mol\ O}_2}{2\mathrm{mol\ HgO}}\rightarrow\frac{32\mathrm{g\ O}_2}{1\mathrm{mol\ O}_2}\\ 2.13\mathrm{g\ HgO}\times\frac{1\mathrm{mol\ HgO}}{216.6\mathrm{g\ HgO}}\times\frac{1\mathrm{mol\ O}_2}{2\mathrm{mol\ HgO}}\times\frac{32\mathrm{g\ O}_2}{1\mathrm{mol\ O}_2}=0.16\mathrm{g\ O}_2\end{array}\)