Chapter 3, Problem 3.135P

(a)

Interpretation Introduction

Interpretation:

The empirical formula of the compound formed when $0.327\text{ g}$ of platinum is heated in fluorine is to be calculated.

Concept introduction:

The empirical formula of a chemical compound is the simplest positive integer ratio of the atoms that are present in the compound. It may or may not be the same as that of the molecular formula. For example, the empirical formula of sulfur dioxide is $\text{SO}$.

(b)

Interpretation Introduction

Interpretation:

The empirical formula of the compound formed when $0.265\text{ g}$ of ${\text{PtF}}_6$ reacts with excess xenon gas is to be determined.

Concept introduction:

The empirical formula of a chemical compound is the simplest positive integer ratio of the atoms that are present in the compound. It may or may not be the same as that of the molecular formula. For example, the empirical formula of sulfur dioxide is $\text{SO}$.

(c)

Interpretation Introduction

Interpretation:

The mass percents of each xenon fluoride in the product mixture are to be determined.

Concept introduction:

Mass percent is employed to determine the concentration of one compound in a mixture of the compound. The formula to calculate mass percent is as follows:

  $\text{Mass percent of compound}=\left(\frac{\text{mass of the compound}}{\text{mass of mixture}}\right)100$