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Chapter 2: Problem 41

Consider 80.0-g samples of two different compounds consisting of only carbon and oxygen. One of the compounds consists of 21.8 g of carbon, and the other has 34.3 g of carbon. Determine the ratio in whole numbers of the masses of carbon that combine with 1.00 g of oxygen between the two compounds.

Short Answer

Expert verified
The ratio in whole numbers of the masses of carbon that combine with 1.00 g of oxygen between the two compounds is 1:2.

Step by step solution

01

Calculate the Mass of Oxygen in Both Compounds

First, we will calculate the mass of oxygen in both compounds. Since the total mass of each compound is 80.0 g, we can find the mass of oxygen in the compounds by subtracting the mass of carbon from the total mass. For the first compound: Mass of oxygen = Total mass - Mass of carbon Mass of oxygen = 80.0 g - 21.8 g = 58.2 g For the second compound: Mass of oxygen = Total mass - Mass of carbon Mass of oxygen = 80.0 g - 34.3 g = 45.7 g
02

Determine the Mass of Carbon that Bonds with 1 g of Oxygen in Both Compounds

Next, we will calculate the mass of carbon that combines with 1 g of oxygen for both compounds. For the first compound: Mass of carbon combined with 1 g of oxygen = (Mass of carbon) / (Mass of oxygen) = 21.8 g / 58.2 g = 0.374 g of carbon For the second compound: Mass of carbon combined with 1 g of oxygen = (Mass of carbon) / (Mass of oxygen) = 34.3 g / 45.7 g = 0.750 g of carbon
03

Calculate the Ratio of the Masses of Carbon that Combine with 1.00 g of Oxygen between the Two Compounds

Finally, we will find the ratio of the masses of carbon that combined with 1.00 g of oxygen between the two compounds. Ratio = (Mass of carbon in the first compound that combined with 1 g of oxygen) / (Mass of carbon in the second compound that combined with 1 g of oxygen) = 0.374 g / 0.750 g ≈ 0.499 Now we need to convert this ratio to whole numbers. For simplicity, we can round it to the nearest whole number: Ratio ≈ 1/2 Therefore, the ratio in whole numbers of the masses of carbon that combine with 1.00 g of oxygen between the two compounds is 1:2.

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Most popular questions from this chapter

Chlorine has two natural isotopes: \(_{17}^{37} \mathrm{Cl}\) and 35 17 \(\mathrm{Cl}\) Hydrogen reacts with chlorine to form the compound HCl. Would a given amount of hydrogen react with different masses of the two chlorine isotopes? Does this conflict with the law of definite proportion? Why or why not?

In an experiment it was found that the total charge on an oil drop was $5.93 \times 10^{-18} \mathrm{C}$ . How many negative charges does the drop contain?

When hydrogen is burned in oxygen to form water, the composition of water formed does not depend on the amount of oxygen reacted. Interpret this in terms of the law of definite proportion.

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What are the symbols for the following nonmetal elements that are most often present in compounds studied in organic chemistry: carbon, hydrogen, oxygen, nitrogen, phosphorus, sulfur? Predict a stable isotope for each of these elements.
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