(Solved): Lithium and nitrogen react in a combination reaction to produce lithium nitride: \( 6 \mathrm{Li}( ...

Lithium and nitrogen react in a combination reaction to produce lithium nitride: \( 6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s) \) In a particular experiment, 1.00-g samples of each reagent are reacted. The theoretical yield of lithium nitride is g. \( 5.0 \) \( 2.50 \) \( 0.84 \) \( 1.01 \) \( 1.67 \) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: \( 2 \mathrm{NaN}_{3}(s) \rightarrow 2 \mathrm{Na}(s)+3 \mathrm{~N}_{2}(g) \) How many moles of \( \mathrm{N}_{2} \) are produced by the decomposition of \( 1.00 \) mol of sodium azide? \( 0.667 \) \( 0.500 \) \( 3.00 \) \( 0.333 \) \( 1.50 \) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: \( 2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{MgO}(s) \) When \( 5.00 \mathrm{~g} \) of magnesium burns, the theoretical yield of magnesium oxide is g. \( 8.29 \) \( 4.15 \) \( 0.206 \) \( 5.00 \) \( 16.6 \) Identify the correct balanced equation for the combustion of propane \( \left(\mathrm{C}_{3} \mathrm{H}_{8}\right) \). \[ \begin{array}{l} \mathrm{C}_{3} \mathrm{H}_{8}(g) \rightarrow 4 \mathrm{H}_{2}(g)+3 \mathrm{C}(s) \\ \mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{H}_{2} \mathrm{O}(g)+3 \mathrm{CO}_{2}(g) \\ \mathrm{C}_{3} \mathrm{H}_{8}(g)+3 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{H}_{2} \mathrm{O}(g)+3 \mathrm{CO}_{2}(g) \\ 2 \mathrm{C}_{3} \mathrm{H}_{8}(g)+9 \mathrm{O}_{2}(g) \rightarrow 6 \mathrm{H}_{2} \mathrm{CO}_{3}(g)+2 \mathrm{H}_{2}(g) \end{array} \] Enter a balanced equation for the complete combustion of liquid \( \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{SH} \). Express your answer as a chemical equation. Identify all of the phases in your answer.