Balance each of the following chemical equations. a. FeCl3(a q)+KOH(a q) →Fe(OH)3(s)+KCl(a q) b.

step 1 So problem 37 is asking us to balance these chemical equations. So this first chemical equation,

Balance each of the following chemical equations. a. FeCl3(a...

Balance each of the following chemical equations. a. $\mathrm{FeCl}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{KCl}(a q)$ b. $\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{KI}(a q) \rightarrow \mathrm{PbI}_{2}(s)+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)$ c. $\mathrm{P}_{4} \mathrm{O}_{10}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)$ d. $\mathrm{Li}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(a q)$ e. $\operatorname{MnO}_{2}(s)+\mathrm{C}(s) \rightarrow \operatorname{Mn}(s)+\mathrm{CO}_{2}(g)$ f. $\mathrm{Sb}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{SbCl}_{3}(s)$ g. $\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)$ h. $\mathrm{FeS}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{~S}(g)$

Balance each of the following chemical equations.
a. $\mathrm{FeCl}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{KCl}(a q)$
b. $\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{KI}(a q) \rightarrow \mathrm{PbI}_{2}(s)+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)$
c. $\mathrm{P}_{4} \mathrm{O}_{10}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)$
d. $\mathrm{Li}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(a q)$
e. $\operatorname{MnO}_{2}(s)+\mathrm{C}(s) \rightarrow \operatorname{Mn}(s)+\mathrm{CO}_{2}(g)$
f. $\mathrm{Sb}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{SbCl}_{3}(s)$
g. $\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)$
h. $\mathrm{FeS}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{~S}(g)$

Key Concepts

State Symbols

State symbols indicate the physical states of the substances in a chemical reaction, using abbreviations such as (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solution. They play an important role in helping to identify the conditions under which reactions occur and can impact the balancing process in more complex chemical systems.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between species, resulting in changes in their oxidation states. Balancing redox reactions not only requires ensuring that the atoms are balanced, but also that the electrons lost in oxidation are equal to those gained in reduction. This often involves additional steps or methods compared to simpler reaction types.

Balancing Chemical Equations

Balancing chemical equations is the process of adjusting the coefficients of reactants and products in a chemical reaction so that the number of atoms for each element is equal on both sides of the equation. This systematic approach ensures that the equation adheres to the law of conservation of mass, providing a clear, quantitative depiction of the chemical process.

Law of Conservation of Mass

This fundamental principle of chemistry states that matter is neither created nor destroyed in a chemical reaction. Every balanced chemical equation must reflect that the total mass (or number of atoms) of the reactants is equal to the total mass (or number of atoms) of the products, ensuring that atoms are simply rearranged, not lost or gained, during the reaction.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It uses the coefficients in a balanced chemical equation to represent the relative number of moles of each substance involved, which is essential for calculating reactant consumption and product formation.