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Chapter 2: Problem 13

Sulfur forms two compounds with oxygen. In the first compound, \(1.000 \mathrm{g}\) sulfur is combined with \(0.998 \mathrm{g}\) oxygen, and in the second, \(1.000 \mathrm{g}\) sulfur is combined with \(1.497 \mathrm{g}\) oxygen. Show that these results are consistent with Dalton's law of multiple proportions

Short Answer

Expert verified
The mass ratios of oxygen to sulfur in the two compounds are approximately 1:1 and 1.5:1. Taylor's law of multiple proportions, which states that these ratios should be small whole numbers, is therefore confirmed by these results, although there is a minor discrepancy, likely due to measurement or rounding errors.

Step by step solution

01

Determine the Ratios

First, the mass ratios of oxygen to sulfur in both compounds need to be determined. This can be done by dividing the mass of the oxygen by the mass of the sulfur. In the first compound, the ratio is \(0.998 \, \mathrm{g} / 1.000 \, \mathrm{g} = 0.998\). In the second compound, the ratio is \(1.497 \, \mathrm{g} / 1.000 \, \mathrm{g} = 1.497\).
02

Compare the Ratios

Next, divide the larger ratio by the smaller ratio. This should give a number that is a small whole number or very close to it if the law of multiple proportions is valid. Hence, \(1.497/0.998 = 1.50\).
03

Interpret the Result

The result of the division yields approximately 1.5. Although this is not a whole number, it is very close to the whole number 1.5, which suggests that the given data are generally consistent with the law of multiple proportions. Small deviations from whole numbers can be due to experimental inaccuracies or rounding errors.

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Most popular questions from this chapter

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