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Chapter 8: Problem 50

Write the balanced equation for each of the following: $$\begin{array}{l}{\text { a. the complete combustion of propane gas, }} \\\ {\mathrm{C}_{3} \mathrm{H}_{8}} \\ {\text { b. the decomposition of magnesium carbonate }} \\ {\text { c. the synthesis of platinum(IV) fluoride }} \\\ {\text { from platinum and fluorine gas }} \\ {\text { d. the reaction of zinc with lead(II) nitrate }}\end{array}$$

Short Answer

Expert verified
The balanced equations for the reactions are: \n(a) \(C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O\)\n(b) \(MgCO_3 \rightarrow MgO + CO_2\)\n(c) \(Pt + 2F_2 \rightarrow PtF_4\)\n(d) \(Zn + Pb(NO_3)_2 \rightarrow Zn(NO_3)_2 + Pb\)

Step by step solution

01

Combustion of Propane Gas

Propane (\(C_3H_8\)) reacts with oxygen gas (\(O_2\)) on burning, producing carbon dioxide (\(CO_2\)) and water (\(H_2O\)). The initial unbalanced equation is \(C_3H_8 + O_2 \rightarrow CO_2 + H_2O\). To balance this:- There are 3 carbons on the left so put a 3 in front of \(CO_2\).- There are 8 hydrogens on the left so put a 4 in front of \(H_2O\).- Lastly, to balance the oxygens, put a 5 in front of \(O_2\). So, the balanced equation is \(C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O\).
02

Decomposition of Magnesium Carbonate

Magnesium carbonate (\(MgCO_3\)) decomposes into magnesium oxide (\(MgO\)) and carbon dioxide (\(CO_2\)). The balanced equation is \(MgCO_3 \rightarrow MgO + CO_2\).
03

Synthesis of Platinum(IV) Fluoride

Platinum (\(Pt\)) reacts with fluorine gas (\(F_2\)) to produce platinum(IV) fluoride (\(PtF_4\)). The initial unbalanced equation is \(Pt + F_2 \rightarrow PtF_4\). To balance it, add a 2 in front of \(F_2\). Thus, the balanced equation is \(Pt + 2F_2 \rightarrow PtF_4\).
04

Reaction of Zinc with Lead(II) Nitrate

Zinc (\(Zn\)) reacts with lead(II) nitrate (\(Pb(NO_3)_2\)) to form zinc nitrate (\(Zn(NO_3)_2\)) and lead (\(Pb\)). Therefore, the balanced equation is \(Zn + Pb(NO_3)_2 \rightarrow Zn(NO_3)_2 + Pb\).

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Most popular questions from this chapter

Define each of the following terms: $$\begin{array}{l}{\text { a. decomposition reaction }} \\ {\text { b. double-displacement reaction }} \\ {\text { c. spectator ions }} \\ {\text { d. activity series }}\end{array}$$

What must form in order for a double-displacement reaction to occur?

Although cesium is not listed in the activity series in this chapter, predict where cesium would appear based on its position in the periodic table.

Identify the type of reaction for each of the following. Then, predict products for the reaction, and balance the equation." reaction occurs, write "no reaction." $$\text{a}. \mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$ $$\text{b}. \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\text{c}. \mathrm{CdCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow 2 \mathrm{NaCl}(a q)+\mathrm{CdCO}_{3}(s)$$

Write the symbol used in a chemical equation to represent each of the following: $$\begin{array}{l}{\text { a. an aqueous solution }} \\ {\text { b. heated }} \\\ {\text { c. a reversible reaction }} \\ {\text { d. a solid }} \\ {\text { e. at a temperature of } 25^{\circ} \mathrm{C}}\end{array}$$
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