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Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang
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Solved: Heating 2.40 g of the oxide of metal X (molar mass

Chapter 3, Problem 139P

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QUESTION:

Heating 2.40 g of the oxide of metal X (molar mass of X = 55.9 g/mol) in carbon monoxide (CO) yields the pure metal and carbon dioxide. The mass of the metal product is 1.68 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.

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QUESTION:

Heating 2.40 g of the oxide of metal X (molar mass of X = 55.9 g/mol) in carbon monoxide (CO) yields the pure metal and carbon dioxide. The mass of the metal product is 1.68 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.

ANSWER:

Step 1 of 3

Here, we are asked to show that the simplest formula of the oxide is  and write a balanced equation for the reaction.

The Empirical formula of a compound is the simplest formula of a compound. It is the simplest positive integer ratio of atoms present in a compound. The smallest whole number ratios of the subscripts of molecular formula are derived by dividing the subscripts by largest common factor.

Example: the empirical formula of disulfur dioxide is .

 the empirical formula of ethane() will be .

 

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