Questions: 1. Using chemical formulas, write the following chemical reaction equations; include the state of matter and balance the equation: a. Nitrogen gas reacts with hydrogen gas to produce ammonia gas. b. Potassium chlorate solid decomposes into potassium chloride solid and oxygen gas. c. Sodium chloride solid reacts with fluorine gas to produce sodium fluoride solid and chlorine gas. d. Lead (II) hydroxide solid reacts with hydrochloric acid in aqueous solution to produce liquid water and lead (II) chloride. e. Nitric acid in aqueous solution reacts with sodium hydrogen carbonate in aqueous solution to produce sodium nitrate in aqueous solution, liquid water and carbon dioxide gas. f. Iron (III) chloride in aqueous solution reacts with sodium hydroxide in aqueous solution to produce solid iron (III) hydroxide and sodium chloride in aqueous solution.

1. Using chemical formulas, write the following chemical reaction equations; include the state of matter and balance the equation: a. Nitrogen gas reacts with hydrogen gas to produce ammonia gas. b. Potassium chlorate solid decomposes into potassium chloride solid and oxygen gas. c. Sodium chloride solid reacts with fluorine gas to produce sodium fluoride solid and chlorine gas. d. Lead (II) hydroxide solid reacts with hydrochloric acid in aqueous solution to produce liquid water and lead (II) chloride. e. Nitric acid in aqueous solution reacts with sodium hydrogen carbonate in aqueous solution to produce sodium nitrate in aqueous solution, liquid water and carbon dioxide gas. f. Iron (III) chloride in aqueous solution reacts with sodium hydroxide in aqueous solution to produce solid iron (III) hydroxide and sodium chloride in aqueous solution.
Transcript text: 1. Using chemical formulas, write the following chemical reaction equations; include the state of matter and balance the equation: a. Nitrogen gas reacts with hydrogen gas to produce ammonia gas. b. Potassium chlorate solid decomposes into potassium chloride solid and oxygen gas. c. Sodium chloride solid reacts with fluorine gas to produce sodium fluoride solid and chlorine gas. d. Lead (II) hydroxide solid reacts with hydrochloric acid in aqueous solution to produce liquid water and lead (II) chloride. e. Nitric acid in aqueous solution reacts with sodium hydrogen carbonate in aqueous solution to produce sodium nitrate in aqueous solution, liquid water and carbon dioxide gas. f. Iron (III) chloride in aqueous solution reacts with sodium hydroxide in aqueous solution to produce solid iron (III) hydroxide and sodium chloride in aqueous solution.
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Solution

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Solution Steps

Step 1: Write the Unbalanced Chemical Equations

First, we write the unbalanced chemical equations for each reaction.

a. \( \text{N}_2(g) + \text{H}_2(g) \rightarrow \text{NH}_3(g) \)

b. \( \text{KClO}_3(s) \rightarrow \text{KCl}(s) + \text{O}_2(g) \)

c. \( \text{NaCl}(s) + \text{F}_2(g) \rightarrow \text{NaF}(s) + \text{Cl}_2(g) \)

d. \( \text{Pb(OH)}_2(s) + \text{HCl}(aq) \rightarrow \text{H}_2\text{O}(l) + \text{PbCl}_2(s) \)

e. \( \text{HNO}_3(aq) + \text{NaHCO}_3(aq) \rightarrow \text{NaNO}_3(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \)

f. \( \text{FeCl}_3(aq) + \text{NaOH}(aq) \rightarrow \text{Fe(OH)}_3(s) + \text{NaCl}(aq) \)

Step 2: Balance the Chemical Equations

Next, we balance each chemical equation.

a. \( \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \)

b. \( 2\text{KClO}_3(s) \rightarrow 2\text{KCl}(s) + 3\text{O}_2(g) \)

c. \( 2\text{NaCl}(s) + \text{F}_2(g) \rightarrow 2\text{NaF}(s) + \text{Cl}_2(g) \)

d. \( \text{Pb(OH)}_2(s) + 2\text{HCl}(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{PbCl}_2(s) \)

e. \( \text{HNO}_3(aq) + \text{NaHCO}_3(aq) \rightarrow \text{NaNO}_3(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \)

f. \( \text{FeCl}_3(aq) + 3\text{NaOH}(aq) \rightarrow \text{Fe(OH)}_3(s) + 3\text{NaCl}(aq) \)

Final Answer

\[ \boxed{ \begin{aligned} \text{a.} & \quad \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \\ \text{b.} & \quad 2\text{KClO}_3(s) \rightarrow 2\text{KCl}(s) + 3\text{O}_2(g) \\ \text{c.} & \quad 2\text{NaCl}(s) + \text{F}_2(g) \rightarrow 2\text{NaF}(s) + \text{Cl}_2(g) \\ \text{d.} & \quad \text{Pb(OH)}_2(s) + 2\text{HCl}(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{PbCl}_2(s) \\ \text{e.} & \quad \text{HNO}_3(aq) + \text{NaHCO}_3(aq) \rightarrow \text{NaNO}_3(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \\ \text{f.} & \quad \text{FeCl}_3(aq) + 3\text{NaOH}(aq) \rightarrow \text{Fe(OH)}_3(s) + 3\text{NaCl}(aq) \end{aligned} } \]

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