Balance each of the following chemical equations. a. Fe3 O4(s)+H2(g) →Fe(l)+H2 O(g) b. K2 SO4(a

step 1 Problem 41 is asking us to balance these equations. So with this first one, you see that we have

Balance each of the following chemical equations. a. Fe3...

Balance each of the following chemical equations. a. $\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{H}_{2}(g) \rightarrow \mathrm{Fe}(l)+\mathrm{H}_{2} \mathrm{O}(g)$ b. $\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{BaCl}_{2}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{KCl}(a q)$ c. $\mathrm{HCl}(a q)+\mathrm{FeS}(s) \rightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{~S}(g)$ d. $\mathrm{Br}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{HBr}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)$ e. $\mathrm{CS}_{2}(l)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{CCl}_{4}(l)+\mathrm{S}_{2} \mathrm{Cl}_{2}(g)$ f. $\mathrm{Cl}_{2} \mathrm{O}_{7}(g)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ g. $\operatorname{PBr}_{3}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}(a q)+\mathrm{HBr}(g)$ h. $\mathrm{Ba}\left(\mathrm{ClO}_{3}\right)_{2}(s) \rightarrow \mathrm{BaCl}_{2}(s)+\mathrm{O}_{2}(s)$

Balance each of the following chemical equations.
a. $\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{H}_{2}(g) \rightarrow \mathrm{Fe}(l)+\mathrm{H}_{2} \mathrm{O}(g)$
b. $\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{BaCl}_{2}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{KCl}(a q)$
c. $\mathrm{HCl}(a q)+\mathrm{FeS}(s) \rightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{~S}(g)$
d. $\mathrm{Br}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{HBr}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)$
e. $\mathrm{CS}_{2}(l)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{CCl}_{4}(l)+\mathrm{S}_{2} \mathrm{Cl}_{2}(g)$
f. $\mathrm{Cl}_{2} \mathrm{O}_{7}(g)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$
g. $\operatorname{PBr}_{3}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}(a q)+\mathrm{HBr}(g)$
h. $\mathrm{Ba}\left(\mathrm{ClO}_{3}\right)_{2}(s) \rightarrow \mathrm{BaCl}_{2}(s)+\mathrm{O}_{2}(s)$

Key Concepts

Conservation of Mass

This principle states that matter is neither created nor destroyed during a chemical reaction. Every atom that appears on the reactants side must appear on the products side, which is the fundamental idea behind balancing chemical equations.

Stoichiometry

Stoichiometry involves calculating the quantitative relationships between reactants and products in a chemical reaction. It uses the balanced equation to determine the proportions of each species involved, ensuring that the law of conservation of mass is satisfied.

Balancing Chemical Equations

Balancing chemical equations is the process of adjusting coefficients in a chemical formula so that the number of atoms for each element is equal on both sides of the equation. This systematic approach reflects the conservation of mass and enables accurate stoichiometric calculations.

Coefficient Adjustment

This concept refers to changing the numerical multipliers in front of the compounds in an equation, rather than altering the chemical formulas themselves. Correctly adjusting these coefficients is essential to ensure that the equation meets atomic balance criteria in accordance with the conservation of mass.