Chapter 20: Problem 36
Write a balanced equation describing the reaction of aluminum metal with concentrated aqueous sodium hydroxide.
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. \(\operatorname{Si} \mathrm{O}_{2}(s)+\mathrm{C}(s) \longrightarrow \mathrm{Si}(s)+\mathrm{CO}(g)\) b. Silicon tetrachloride is reacted with very pure magne- sium, producing silicon and magnesium chloride. c. \(\mathrm{Na}_{2} \mathrm{SiF}_{6}(s)+\mathrm{Na}(s) \longrightarrow \mathrm{Si (s)+\mathrm{NaF}(s)\)
Arsenic reacts with oxygen to form oxides that react with water in a manner analogous to that of the phosphorus oxides. Write balanced chemical equations describing the reaction of arsenic with oxygen and the reaction of the resulting oxide with water.
The compound with the formula TII_ is a black solid. Given the following standard reduction potentials, \(\mathrm{T} 1^{3+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Tl}^{+}\) \(\mathscr{E}^{\circ}=1.25 \mathrm{V}\) \(\mathrm{I}_{3}^{-}+2 \mathrm{e}^{-} \longrightarrow 3 \mathrm{I}^{-}\) \(\mathscr{E}^{\circ}=0.55 \mathrm{V}\)
Nitrous oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) can be produced by thermal decomposition of ammonium nitrate: $$ \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \stackrel{\mathrm{heat}}{\longrightarrow} \mathrm{N}_{2} \mathrm{O}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ What volume of \(\mathrm{N}_{2} \mathrm{O}(g)\) collected over water at a total pressure of 94.0 \(\mathrm{kPa}\) and \(22^{\circ} \mathrm{C}\) can be produced from thermal decomposition of 8.68 \(\mathrm{g} \mathrm{NH}_{4} \mathrm{NO}_{3} ?\) The vapor pressure of water at \(22^{\circ} \mathrm{C}\) is 21 torr.
Fluorine reacts with sulfur to form several different covalent compounds. Three of these compounds are \(\mathrm{SF}_{2}, \mathrm{SF}_{4},\) and \(\mathrm{SF}_{6} .\) Draw the Lewis structures for these compounds, and predict the molecular structures (including bond angles). Would you expect \(\mathrm{OF}_{4}\) to be a stable compound?
What do you think about this solution?
We value your feedback to improve our textbook solutions.
