Answer
a. \( 6\operatorname{Li}(s)+\mathrm{N}_{2}(g) \rightarrow 2\operatorname{Li}_{3}\mathrm{N}(s) \)
b. \( 2\mathrm{Rb}(s)+\mathrm{S}(s) \rightarrow \mathrm{Rb}_{2}\mathrm{S}(s) \)
Work Step by Step
Let's explain the balanced equations:
a. \( 6\operatorname{Li}(s)+\mathrm{N}_{2}(g) \rightarrow 2\operatorname{Li}_{3}\mathrm{N}(s) \)
In this reaction, 6 atoms of lithium (\( \operatorname{Li} \)) react with 1 molecule of nitrogen (\( \mathrm{N}_{2} \)) to form 2 molecules of lithium nitride (\( \operatorname{Li}_{3}\mathrm{N} \)). The balanced equation ensures that the same number of each type of atom is present on both sides of the equation.
b. \( 2\mathrm{Rb}(s)+\mathrm{S}(s) \rightarrow \mathrm{Rb}_{2}\mathrm{S}(s) \)
In this reaction, 2 atoms of rubidium (\( \mathrm{Rb} \)) react with 1 atom of sulfur (\( \mathrm{S} \)) to form 1 molecule of rubidium sulfide (\( \mathrm{Rb}_{2}\mathrm{S} \)). Again, the balanced equation ensures that the same number of each type of atom is present on both sides of the equation.
Balancing chemical equations is important because it reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
