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Chapter 5: Problem 91

One of the components that make up common table sugar is fructose, a compound that contains only carbon, hydrogen, and oxygen. Complete combustion of \(1.50 \mathrm{g}\) of fructose produced \(2.20 \mathrm{g}\) of carbon dioxide and \(0.900 \mathrm{g}\) of water. What is the empirical formula of fructose?

Short Answer

Expert verified
The empirical formula of fructose is CH₂O.

Step by step solution

01

Calculate the moles of carbon dioxide and water produced

Given that 2.20 g of carbon dioxide (CO₂) and 0.900 g of water (H₂O) are produced, we will first convert these masses into moles. Molar mass of CO₂ = 12.01 g/mol (C) + 2 × 16.00 g/mol (O) = 44.01 g/mol Molar mass of H₂O = 2 × 1.01 g/mol (H) + 16.00 g/mol (O) = 18.02 g/mol Moles of CO₂ = mass of CO₂ / molar mass of CO₂ = 2.20 g / 44.01 g/mol = 0.0500 mol Moles of H₂O = mass of H₂O / molar mass of H₂O = 0.900 g / 18.02 g/mol = 0.0500 mol
02

Determine the mass of carbon and hydrogen present in fructose

Knowing the moles of CO₂ and H₂O produced, we can calculate the mass of carbon (from CO₂) and hydrogen (from H₂O) in fructose. Mass of Carbon = moles of CO₂ × molar mass of C = 0.0500 mol × 12.01 g/mol = 0.600 g Mass of Hydrogen = moles of H₂O × (2 × molar mass of H) = 0.0500 mol × (2 × 1.01 g/mol) = 0.101 g (rounded)
03

Calculate the mass of oxygen present in fructose

The total mass of fructose is given as 1.50 g. We can determine the mass of oxygen in fructose by subtracting the masses of carbon and hydrogen from the total mass. Mass of Oxygen = 1.50 g - (0.600 g + 0.101 g) = 0.799 g (rounded)
04

Convert the masses of carbon, hydrogen, and oxygen into moles

Now, let's convert the masses of carbon, hydrogen, and oxygen to moles using their molar masses. Moles of Carbon = mass of Carbon / molar mass of C = 0.600 g / 12.01 g/mol = 0.0500 mol Moles of Hydrogen = mass of Hydrogen / molar mass of H = 0.101 g / 1.01 g/mol ≈ 0.100 mol Moles of Oxygen = mass of Oxygen / molar mass of O = 0.799 g / 16.00 g/mol ≈ 0.0500 mol
05

Find the ratio of the moles of each element and determine the empirical formula

To find the empirical formula, we will divide the moles of each element by the smallest number of moles, and then round each value to the nearest whole number. Ratio of C: 0.0500 mol / 0.0500 mol = 1 Ratio of H: 0.100 mol / 0.0500 mol = 2 Ratio of O: 0.0500 mol / 0.0500 mol = 1 So the empirical formula of fructose is CH₂O.

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Most popular questions from this chapter

Some bismuth tablets, a medication used to treat upset stomachs, contain \(262 \mathrm{mg}\) of bismuth subsalicylate, \(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{BiO}_{4},\) per tablet. Assuming two tablets are digested, calculate the mass of bismuth consumed.

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