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Chapter 2: Problem 46

In a combustion reaction, 46.0 g of ethanol reacts with 96.0 g of oxygen to produce water and carbon dioxide. If 54.0 g of water is produced, what mass of carbon dioxide is produced?

Short Answer

Expert verified
The mass of carbon dioxide produced in the combustion of ethanol is 88.0 g.

Step by step solution

01

Write the balanced chemical equation for the combustion of ethanol.

The combustion of ethanol (C2H5OH) with oxygen (O2) produces water (H2O) and carbon dioxide (CO2). To balance the equation, we must ensure that there are the same number of atoms of each element on both sides of the equation: C2H5OH + O2 -> H2O + CO2 Balanced equation: C2H5OH + 3O2 -> 2H2O + 2CO2
02

Calculate the moles of ethanol and oxygen

First, we need to find the moles of ethanol and oxygen present in the reaction. To do this, we will use the given masses and the molar masses of ethanol and oxygen. Given mass of ethanol: 46.0 g Molar mass of ethanol: 12.01 g/mol (C) * 2 + 1.01 g/mol (H) * 6 + 16.00 g/mol (O) = 46.07 g/mol Moles of ethanol = mass of ethanol / molar mass of ethanol = 46.0 g / 46.07 g/mol ≈ 1.0 mol Given mass of oxygen: 96.0 g Molar mass of oxygen: 16.00 g/mol (O) * 2 = 32.00 g/mol Moles of oxygen = mass of oxygen / molar mass of oxygen = 96.0 g / 32.00 g/mol = 3.0 mol
03

Identify the limiting reactant

Now, we can determine which reactant is the limiting reactant. The reactant that produces fewer moles of product is the limiting reactant. Based on the balanced chemical equation, 1 mole of ethanol reacts with 3 moles of oxygen. Ratio of moles of ethanol to moles of oxygen: 1.0 mol / 3.0 mol = 1/3 Since the ratio matches the stoichiometric ratio in the balanced equation, there is no excess reactant, and both reactants are completely consumed in the reaction.
04

Calculate the moles of carbon dioxide produced

Now, we can use stoichiometry to determine the moles of carbon dioxide produced in the reaction. According to the balanced equation, 1 mole of ethanol produces 2 moles of carbon dioxide: 1.0 mol ethanol * (2 mol CO2 / 1 mol ethanol) = 2.0 mol CO2
05

Calculate the mass of carbon dioxide produced

Finally, we can convert the moles of carbon dioxide produced to mass using its molar mass: Molar mass of carbon dioxide: 12.01 g/mol (C) + 16.00 g/mol (O) * 2 = 44.01 g/mol Mass of carbon dioxide = moles of carbon dioxide * molar mass of carbon dioxide = 2.0 mol * 44.01 g/mol = 88.0 g
06

Answer

The mass of carbon dioxide produced in the combustion of ethanol is 88.0 g.

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Most popular questions from this chapter

The designations 1A through 8A used for certain families of the periodic table are helpful for predicting the charges on ions in binary ionic compounds. In these compounds, the metals generally take on a positive charge equal to the family number, while the nonmetals take on a negative charge equal to the family number minus eight. Thus the compound between sodium and chlorine contains \(\mathrm{Na}^{+}\) ions and \(\mathrm{Cl}^{-}\) ions and has the formula NaCl. Predict the formula and the name of the binary compound formed from the following pairs of elements. a. Ca and N b. \(\mathrm{K}\) and \(\mathrm{O}\) c. \(\mathrm{Rb}\) and \(\mathrm{F}\) d. Mg and S e. Ba and I f. Al and Se g. \(\mathrm{Cs}\) and \(\mathrm{P}\) h. In and Br

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