Balance each of the following chemical equations. a. Ba(NO3)2(a q)+Na2 CrO4(a q) →BaCrO4(s)+NaNO

step 1 Problem 44 is asking us to balance these chemical equations. So let's look at this first one. So

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

Balance each of the following chemical equations. a. $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q) \rightarrow \mathrm{BaCrO}_{4}(s)+\mathrm{NaNO}_{3}(a q)$ b. $\mathrm{PbCl}_{2}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{PbSO}_{4}(s)+\mathrm{KCl}(a q)$ c. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ d. $\mathrm{CaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{C}_{2} \mathrm{H}_{2}(g)$ e. $\operatorname{Sr}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)$ f. $\mathrm{BaO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)$ g. $\operatorname{AsI}_{3}(s) \rightarrow \operatorname{As}(s)+\mathrm{I}_{2}(s)$ h. $\mathrm{CuSO}_{4}(a q)+\mathrm{KI}(s) \rightarrow \mathrm{CuI}(s)+\mathrm{I}_{2}(s)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)$

Balance each of the following chemical equations.
a. $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q) \rightarrow \mathrm{BaCrO}_{4}(s)+\mathrm{NaNO}_{3}(a q)$
b. $\mathrm{PbCl}_{2}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{PbSO}_{4}(s)+\mathrm{KCl}(a q)$
c. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
d. $\mathrm{CaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{C}_{2} \mathrm{H}_{2}(g)$
e. $\operatorname{Sr}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)$
f. $\mathrm{BaO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)$
g. $\operatorname{AsI}_{3}(s) \rightarrow \operatorname{As}(s)+\mathrm{I}_{2}(s)$
h. $\mathrm{CuSO}_{4}(a q)+\mathrm{KI}(s) \rightarrow \mathrm{CuI}(s)+\mathrm{I}_{2}(s)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)$

Key Concepts

Reaction Types

Understanding different reaction types, such as synthesis, decomposition, single replacement, combustion, and precipitation, provides context for balancing equations. Recognizing the type of reaction can guide the balancing process, as certain reactions may have characteristic patterns or require additional considerations related to the states of the reactants and products.

Balancing Chemical Equations

Balancing chemical equations is the process of adjusting the coefficients of reactants and products to ensure that the number of atoms of every element is the same on both sides of the equation. This process is critical in accurately representing how substances react and transform, serving as a foundation for further quantitative analysis in chemistry.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species and require a careful balance of both atoms and charges. Special techniques, such as tracking oxidation states or using the half-reaction method, are sometimes employed to balance these equations correctly, ensuring that both the mass and charge remain conserved.

Law of Conservation of Mass

This fundamental principle of chemistry states that matter is neither created nor destroyed in a chemical reaction. When balancing equations, it ensures that the number of atoms for each element on the reactant side equals the number on the product side, underscoring the necessity for maintaining mass balance throughout the reaction.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It involves determining the correct proportions of substances through stoichiometric coefficients, which are used in balancing chemical equations to reflect the conservation of atoms and mass in the reaction.