Solution Found!
For the reaction shown, calculate how many moles of NO2 form when each amount of
Chapter 8, Problem 17P(choose chapter or problem)
For the reaction shown, calculate how many moles of \(\mathrm{NO}_{2}\) form when each amount of reactant completely reacts.
\(2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)\)
(a) 1.3 mol \(\mathrm{N}_{2} \mathrm{O}_{5}\)
(b) 5.8 mol \(\mathrm{N}_{2} \mathrm{O}_{5}\)
(c) \(4.45 \times 10^{3} \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{5}\)
(d) \(1.006 \times 10^{-3} \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{5}\)
Questions & Answers
QUESTION:
For the reaction shown, calculate how many moles of \(\mathrm{NO}_{2}\) form when each amount of reactant completely reacts.
\(2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)\)
(a) 1.3 mol \(\mathrm{N}_{2} \mathrm{O}_{5}\)
(b) 5.8 mol \(\mathrm{N}_{2} \mathrm{O}_{5}\)
(c) \(4.45 \times 10^{3} \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{5}\)
(d) \(1.006 \times 10^{-3} \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{5}\)
ANSWER:Step 1 of 5
Given the chemical reaction
\(2\mathrm{\ N}_2\mathrm{O}_5(\mathrm{g})\ \rightarrow\ 4\mathrm{\ NO}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g})\)
We are asked to calculate how many moles of \(\mathrm{NO}_{2}\) form when each amount of reactant completely reacts.