Balance each of the following chemical equations. a. KO2(s)+H2 O(l) →KOH(a q)+O2(g)+H2 O2(a q) b

step 1 Alright so we are asked to balance the equation. Let's start with the first one. We have the rea

Balance each of the following chemical equations. a....

Balance each of the following chemical equations. a. $\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{KOH}(a q)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)$ b. $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ c. $\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ d. $\mathrm{PCl}_{5}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{HCl}(g)$ e. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ f. $\mathrm{CaO}(s)+\mathrm{C}(s) \rightarrow \mathrm{CaC}_{2}(s)+\mathrm{CO}_{2}(g)$ g. $\operatorname{MoS}_{2}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{MoO}_{3}(s)+\mathrm{SO}_{2}(g)$ h. $\mathrm{FeCO}_{3}(s)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}(a q)$

Balance each of the following chemical equations.
a. $\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{KOH}(a q)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)$
b. $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$
d. $\mathrm{PCl}_{5}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{HCl}(g)$
e. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
f. $\mathrm{CaO}(s)+\mathrm{C}(s) \rightarrow \mathrm{CaC}_{2}(s)+\mathrm{CO}_{2}(g)$
g. $\operatorname{MoS}_{2}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{MoO}_{3}(s)+\mathrm{SO}_{2}(g)$
h. $\mathrm{FeCO}_{3}(s)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}(a q)$

Key Concepts

Redox Reactions

Redox reactions, or oxidation-reduction reactions, involve the transfer of electrons between chemical species, which results in changes in their oxidation states. Balancing these reactions sometimes requires additional care to ensure that the number of electrons lost in oxidation equals the number of electrons gained in reduction.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It is used to determine the relative quantities of substances involved in the reaction by using the balanced chemical equation as a guide for the mole-to-mole conversion between compounds.

Half-Reaction Method

The half-reaction method is a systematic approach often used to balance redox reactions. It involves splitting the overall chemical reaction into two separate half-reactions—one for oxidation and one for reduction—balancing each individually (including atoms and charge), and then combining them to form the balanced overall reaction.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is equal on both the reactant and product sides of a chemical equation. This reflects the conservation of matter and requires adjusting the stoichiometric coefficients in front of compounds or elements to satisfy the law of conservation of mass.

Conservation of Mass

The principle of conservation of mass states that matter can neither be created nor destroyed during a chemical reaction. This means that the total mass of the reactants must equal the total mass of the products, which is why balancing equations is critical in chemical reactions.