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Chapter 3: Problem 38

If we know the empirical formula of a compound, what additional information do we need to determine its molecular formula?

Short Answer

Expert verified
To find the molecular formula from the empirical formula, additional information needed is the molar mass of the compound.

Step by step solution

01

Understanding Empirical Formula

The empirical formula of a compound represents the simplest ratio of the elements present in it. For example, the empirical formula of Benzene is CH, which means the elements Carbon (C) and Hydrogen (H) are present in the simplest ratio 1:1.
02

Need for Molecular Formula

The molecular formula of a compound represents the actual number of atoms of each element present in one molecule of the compound. In the example of Benzene, the molecular formula is C6H6 which represents that in one molecule of Benzene, there are 6 Carbon atoms and 6 Hydrogen atoms.
03

Identifying the Additional Information Needed

To determine the molecular formula from the empirical formula, it's necessary to know the molar mass of the compound. If we divide the molar mass of the compound by the molar mass implied by the empirical formula, we'll get the factor to multiply the empirical formula to determine the molecular formula.

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Most popular questions from this chapter

Heating \(2.40 \mathrm{~g}\) of the oxide of metal \(\mathrm{X}\) (molar mass of \(X=55.9 \mathrm{~g} / \mathrm{mol}\) ) in carbon monoxide \((\mathrm{CO})\) yields the pure metal and carbon dioxide. The mass of the metal product is \(1.68 \mathrm{~g}\). From the data given, show that the simplest formula of the oxide is \(\mathrm{X}_{2} \mathrm{O}_{3}\) and write a balanced equation for the reaction.

Why is the actual yield of a reaction almost always smaller than the theoretical yield?

Cinnamic alcohol is used mainly in perfumery, particularly in soaps and cosmetics. Its molecular formula is \(\mathrm{C}_{9} \mathrm{H}_{10} \mathrm{O}\) (a) Calculate the percent composition by mass of \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{O}\) in cinnamic alcohol. (b) How many molecules of cinnamic alcohol are contained in a sample of mass \(0.469 \mathrm{~g} ?\)

What are the empirical formulas of the compounds with the following compositions? (a) 40.1 percent \(\mathrm{C}\) 6.6 percent \(\mathrm{H}, 53.3\) percent \(\mathrm{O}\) (b) 18.4 percent \(\mathrm{C}\) 21.5 percent \(\mathrm{N}, 60.1\) percent \(\mathrm{K}\)

Why is the theoretical yield of a reaction determined only by the amount of the limiting reagent?
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