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Chapter 2: Problem 55

These phosphorus sulfides are known: \(\mathrm{P}_{4} \mathrm{~S}_{3}, \mathrm{P}_{4} \mathrm{~S}_{7}\) and \(\mathrm{P}_{4} \mathrm{~S}_{10}\). Do these compounds obey the law of multiple proportions?

Short Answer

Expert verified
The compounds obey the law of multiple proportions if the ratios of the masses of sulfur that combine with a fixed mass of phosphorus are in simple whole numbers.

Step by step solution

01

Calculate the mass of sulfur in each compound

Since the atomic mass of \(P\) (Phosphorus) is 31 and the atomic mass of \(S\) (Sulfur) is 32, calculate the mass of sulfur for each of the three compounds: \(P_{4}S_{3}\), \(P_{4}S_{7}\), and \(P_{4}S_{10}\). The formula to calculate the mass of sulfur for each mole of phosphorus is: \(MassSuppress = \frac{NumberSupRatio * AtomicMassSup}{AtimicMassSup}\), where NumberSupRatio is 3, 7 or 10.
02

Compute the ratios

Compute the ratios of the masses of sulfur in the different formulas. This is done by dividing the mass of sulfur in one compound by the mass of sulfur in another compound.
03

Determine if the compounds obey the law

If the ratios of the masses of sulfur are in simple whole numbers, then the compounds obey the law of multiple proportions. If not, then the compounds do not obey the law of multiple proportions.

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Most popular questions from this chapter

A monatomic ion has a charge of +2 . The nucleus of the parent atom has a mass number of \(55 .\) If the number of neutrons in the nucleus is 1.2 times that of the number of protons, what is the name and symbol of the element?

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