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Chapter 3: Problem 18

(a) When a compound containing \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{O}\) is completely combusted in air, what reactant besides the hydrocarbon is involved in the reaction? (b) What products form in this reaction? (c) What is the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l),\) in air?

Short Answer

Expert verified
(a) The reactant besides the hydrocarbon involved in the combustion process is oxygen (O2). (b) The products formed during the combustion process are carbon dioxide (CO2) and water (H2O). (c) The sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone, C3H6O, in air is 10.5.

Step by step solution

01

a) Identifying the reactant

In a complete combustion reaction, the hydrocarbon reacts with oxygen (O2) from the air. Therefore, the reactant besides the hydrocarbon involved in the reaction is oxygen (O2).
02

b) Identifying the products

In a complete combustion reaction involving a hydrocarbon containing C, H, and O, the products formed are carbon dioxide (CO2) and water (H2O).
03

c) Balancing the chemical equation and finding the sum of coefficients

To find the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone (C3H6O) in air, we first write the unbalanced equation and then balance it. Unbalanced equation: \[C_{3}H_{6}O(l) + O_{2}(g) \rightarrow CO_{2}(g) + H_{2}O(l)\] Now, we balance the equation: \[C_{3}H_{6}O(l) + \frac{7}{2}O_{2}(g) \rightarrow 3CO_{2}(g) + 3H_{2}O(l)\] To find the sum of coefficients for the balanced equation, we add all the coefficients together, including the coefficients of fractions: Sum of coefficients = 1 (C3H6O) + 7/2 (O2) + 3 (CO2) + 3 (H2O) = 1 + 7/2 + 3 + 3 = 1 + 3.5 + 3 + 3 = 10.5 Therefore, the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone in air is 10.5.

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Most popular questions from this chapter

The semiconductor gallium arsenide, GaAs, is used in high-speed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 \(\mathrm{g} / \mathrm{m}^{3} .\) It can be made by reacting trimethylgallium, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{Ga},\) with arsine gas, \(\mathrm{AsH}_{3}\) . The other product of the reaction is methane, \(\mathrm{CH}_{4}\) . (a) If you reacted 450.0 g of trimethylgallium with 300.0 \(\mathrm{g}\) of arsine, what mass of GaAs could you make? (b) Which reactant, if any, would be left over, and how many moles of the leftover reactant would remain? (c) One application of GaAs uses it as a thin film. If you take the mass of GaAs from part (a) and make a 40 -nm thin film from it, what area, in \(\mathrm{cm}^{2},\) would it cover? Recall that \(1 \mathrm{nm}=1 \times 10^{-9} \mathrm{m} .\)

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Sodium hydroxide reacts with carbon dioxide as follows: $$ 2 \mathrm{NaOH}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) $$ Which is the limiting reactant when 1.85 mol \(\mathrm{NaOH}\) and 1.00 \(\mathrm{mol} \mathrm{CO}_{2}\) are allowed to react? How many moles of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) can be produced? How many moles of the excess reactant remain after the completion of the reaction?

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Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: $$ \begin{array}{l}{\text { (a) } \mathrm{C}_{3} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)} \\ {\text { (b) } \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g)} \\ {\text { (c) } \mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)} \\ {\text { (d) } \mathrm{N}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{NH}_{3}(g)} \\\ {\text { (e) } \mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{KOH}(a q)}\end{array} $$
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