49 Balancing Chemical Equations Worksheets [with Answers] - Free Printable

Here are the solutions to the worksheet problems.

1. Balance the following equations and indicate the type of reaction

a. $2\text{Cu}_{(s)} + \text{O}_{2(g)} \rightarrow 2\text{CuO}_{(s)}$
* Type: Formation (Synthesis)

b. $2\text{H}_2\text{O}_{(l)} \rightarrow 2\text{H}_{2(g)} + \text{O}_{2(g)}$
* Type: Decomposition

c. $3\text{Fe}_{(s)} + 4\text{H}_2\text{O}_{(g)} \rightarrow 4\text{H}_{2(g)} + \text{Fe}_3\text{O}_{4(s)}$
* Type: Single Replacement

d. $2\text{AsCl}_{3(aq)} + 3\text{H}_2\text{S}_{(aq)} \rightarrow \text{As}_2\text{S}_{3(s)} + 6\text{HCl}_{(aq)}$
* Type: Double Replacement

e. $\text{CuSO}_4 \cdot 5\text{H}_2\text{O}_{(s)} \rightarrow \text{CuSO}_{4(s)} + 5\text{H}_2\text{O}_{(g)}$
* Type: Decomposition

f. $\text{Fe}_2\text{O}_{3(s)} + 3\text{H}_{2(g)} \rightarrow 2\text{Fe}_{(s)} + 3\text{H}_2\text{O}_{(l)}$
* Type: Single Replacement

g. $\text{CaCO}_{3(s)} \rightarrow \text{CaO}_{(s)} + \text{CO}_{2(g)}$
* Type: Decomposition

h. $8\text{Fe}_{(s)} + \text{S}_{8(s)} \rightarrow 8\text{FeS}_{(s)}$
* Type: Formation (Synthesis)

i. $\text{H}_2\text{S}_{(aq)} + 2\text{KOH}_{(aq)} \rightarrow 2\text{H}_2\text{O}_{(l)} + \text{K}_2\text{S}_{(aq)}$
* Type: Double Replacement (Neutralization)

j. $2\text{NaCl}_{(l)} \rightarrow 2\text{Na}_{(l)} + \text{Cl}_{2(g)}$
* Type: Decomposition

k. $2\text{Al}_{(s)} + 3\text{H}_2\text{SO}_{4(aq)} \rightarrow 3\text{H}_{2(g)} + \text{Al}_2(\text{SO}_4)_{3(aq)}$
* Type: Single Replacement

l. $\text{H}_3\text{PO}_{4(aq)} + 3\text{NH}_4\text{OH}_{(aq)} \rightarrow 3\text{H}_2\text{O}_{(l)} + (\text{NH}_4)_3\text{PO}_{4(aq)}$
* Type: Double Replacement (Neutralization)

m. $\text{C}_3\text{H}_{8(g)} + 5\text{O}_{2(g)} \rightarrow 3\text{CO}_{2(g)} + 4\text{H}_2\text{O}_{(l)}$
* Type: Hydrocarbon Combustion

n. $4\text{Al}_{(s)} + 3\text{O}_{2(g)} \rightarrow 2\text{Al}_2\text{O}_{3(s)}$
* Type: Formation (Synthesis)

o. $\text{CH}_{4(g)} + 2\text{O}_{2(g)} \rightarrow \text{CO}_{2(g)} + 2\text{H}_2\text{O}_{(l)}$
* Type: Hydrocarbon Combustion

p. $\text{K}_2\text{SO}_{4(aq)} + \text{BaCl}_{2(aq)} \rightarrow 2\text{KCl}_{(aq)} + \text{BaSO}_{4(s)}$
* Type: Double Replacement

q. $\text{C}_5\text{H}_{12(l)} + 8\text{O}_{2(g)} \rightarrow 5\text{CO}_{2(g)} + 6\text{H}_2\text{O}_{(g)}$
* Type: Hydrocarbon Combustion

r. $\text{Ca(OH)}_{2(aq)} + 2\text{NH}_4\text{Cl}_{(aq)} \rightarrow 2\text{NH}_4\text{OH}_{(aq)} + \text{CaCl}_{2(aq)}$
* Type: Double Replacement

s. $\text{V}_2\text{O}_{5(s)} + 5\text{Ca}_{(s)} \rightarrow 5\text{CaO}_{(s)} + 2\text{V}_{(s)}$
* Type: Single Replacement

t. $2\text{Na}_{(s)} + \text{ZnI}_{2(aq)} \rightarrow 2\text{NaI}_{(aq)} + \text{Zn}_{(s)}$
* Type: Single Replacement

u. $2\text{C}_7\text{H}_6\text{O}_{3(l)} + 15\text{O}_{2(g)} \rightarrow 14\text{CO}_{2(g)} + 6\text{H}_2\text{O}_{(l)}$
* Type: Other (Combustion of an oxygenated compound)

v. $3\text{Ca}_{(s)} + \text{N}_{2(g)} \rightarrow \text{Ca}_3\text{N}_{2(s)}$
* Type: Formation (Synthesis)

w. $\text{Fe}_2\text{O}_{3(s)} + 3\text{H}_{2(g)} \rightarrow 2\text{Fe}_{(s)} + 3\text{H}_2\text{O}_{(l)}$
* Type: Single Replacement

x. $2\text{C}_{15}\text{H}_{30(l)} + 45\text{O}_{2(g)} \rightarrow 30\text{CO}_{2(g)} + 30\text{H}_2\text{O}_{(g)}$
*(Note: Can be simplified to $1, 22.5, 15, 15$ but whole numbers are preferred)*
* Type: Hydrocarbon Combustion

y. $2\text{BN}_{(s)} + 3\text{F}_{2(g)} \rightarrow 2\text{BF}_{3(s)} + \text{N}_{2(g)}$
* Type: Single Replacement

z. $2\text{C}_{12}\text{H}_{26(l)} + 37\text{O}_{2(g)} \rightarrow 24\text{CO}_{2(g)} + 26\text{H}_2\text{O}_{(g)}$
* Type: Hydrocarbon Combustion

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2. Predict products, states, reaction type, and balance

a. Lead (II) nitrate + Sodium iodide
* Equation: $\text{Pb(NO}_3)_{2(aq)} + 2\text{NaI}_{(aq)} \rightarrow \text{PbI}_{2(s)} + 2\text{NaNO}_{3(aq)}$
* Type: Double Replacement (Precipitation)

b. Zinc sulfide + Oxygen
* Equation: $2\text{ZnS}_{(s)} + 3\text{O}_{2(g)} \rightarrow 2\text{ZnO}_{(s)} + 2\text{SO}_{2(g)}$
* Type: Other (Roasting/Combustion)

c. Butane combustion
* Equation: $2\text{C}_4\text{H}_{10(l)} + 13\text{O}_{2(g)} \rightarrow 8\text{CO}_{2(g)} + 10\text{H}_2\text{O}_{(g)}$
* Type: Hydrocarbon Combustion

d. Barium hydroxide + Hydrochloric acid
* Equation: $\text{Ba(OH)}_{2(aq)} + 2\text{HCl}_{(aq)} \rightarrow 2\text{H}_2\text{O}_{(l)} + \text{BaCl}_{2(aq)}$
* Type: Double Replacement (Neutralization)

e. Copper + Silver nitrate
* Equation: $\text{Cu}_{(s)} + 2\text{AgNO}_{3(aq)} \rightarrow \text{Cu(NO}_3)_{2(aq)} + 2\text{Ag}_{(s)}$
* Type: Single Replacement

f. Sulfur + Oxygen
* Equation: $\text{S}_{(s)} + \text{O}_{2(g)} \rightarrow \text{SO}_{2(g)}$
* Type: Formation (Synthesis)

g. Aluminum sulfate + Calcium hydroxide
* Equation: $\text{Al}_2(\text{SO}_4)_{3(aq)} + 3\text{Ca(OH)}_{2(aq)} \rightarrow 2\text{Al(OH)}_{3(s)} + 3\text{CaSO}_{4(s)}$
* Type: Double Replacement (Precipitation)

h. Zinc + Sulfuric acid
* Equation: $\text{Zn}_{(s)} + \text{H}_2\text{SO}_{4(aq)} \rightarrow \text{ZnSO}_{4(aq)} + \text{H}_{2(g)}$
* Type: Single Replacement

i. Aluminum + Chlorine gas
* Equation: $2\text{Al}_{(s)} + 3\text{Cl}_{2(g)} \rightarrow 2\text{AlCl}_{3(s)}$
* Type: Formation (Synthesis)

j. Sucrose cellular respiration
* Equation: $\text{C}_{12}\text{H}_{22}\text{O}_{11(s)} + 12\text{O}_{2(g)} \rightarrow 12\text{CO}_{2(g)} + 11\text{H}_2\text{O}_{(l)}$
* Type: Hydrocarbon Combustion (Respiration)