Chapter 6, Problem 11STP

Interpretation Introduction

Interpretation: The true and false statements for the determination of empirical formula of compound needs to be determined.

Concept Introduction: The molecular mass of compound is the sum of atomic mass of all the atoms present in the given chemical compound. Here the molecular formula represents the exact number of all bonded atoms in the compound.

Whereas empirical formula can be defined as the simplest positive integer ratio of all bonded atoms in the compound.

Explanation of Solution

Reason for true statements: Statement A is only true statement.

To calculate the mole of each element, the mass percentage should be considered as the mass of each element. Therefore the mass of compound should be considered as 100.0 g.

Conclusion

Reason for false statements: Statement B, C and D are false statements.

Explanation: The mass percent of each element must be converted to moles not to relative number of atoms. The moles of each element must be divided with least moles to get the smallest percent by mass. The empirical formula can be determined without molar mass as it just requires the mass percentage or moles of each element.

Molecular formula can be determined with the help of molar mass and empirical formula.