The general empirical formula of the compound that contains carbon and hydrogen has to be determined. Concept introduction: The molecular formula signifies the number of atoms corresponding to each of the elements found in a molecule. Empirical formula denotes the simplified ratio of atoms corresponding to each of the element found in a molecule. The empirical formula for a compound when amount of CO 2 and H 2 O are given as follows: The number of moles of the elements is the fractional amounts so write the number of moles of each element as the subscript of the element’s symbol to obtain a preliminary formula for the compound. Convert the moles corresponding to each of the elements to the whole number subscripts. The steps for this conversion are given as follows: (a) Each subscript is divided by the value of smallest digit found in the subscript. (b) If the whole number is not obtained after division, multiply the obtained subscripts by the smallest integer. This gives empirical formula of the compound. Add molar mass corresponding to each of the element multiplied by its number of atoms present in the empirical formula to obtain empirical formula mass for the compound.

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Chapter 6, Problem 6.134QE

Interpretation Introduction

Interpretation:

The general empirical formula of the compound that contains carbon and hydrogen has to be determined.

Concept introduction:

The molecular formula signifies the number of atoms corresponding to each of the elements found in a molecule. Empirical formula denotes the simplified ratio of atoms corresponding to each of the element found in a molecule.

The empirical formula for a compound when amount of CO2 and H2O are given as follows:

The number of moles of the elements is the fractional amounts so write the number of moles of each element as the subscript of the element’s symbol to obtain a preliminary formula for the compound.

Convert the moles corresponding to each of the elements to the whole number subscripts. The steps for this conversion are given as follows:

(a) Each subscript is divided by the value of smallest digit found in the subscript.

(b) If the whole number is not obtained after division, multiply the obtained subscripts by the smallest integer. This gives empirical formula of the compound.

Add molar mass corresponding to each of the element multiplied by its number of atoms present in the empirical formula to obtain empirical formula mass for the compound.

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