   Chapter 3, Problem 137AE

Chapter
Section
Textbook Problem

A given sample of a xenon fluoride compound contains molecules of the type XeFn, where n is some whole number. Given that 9.03 × 1020 molecules of XeFn. weigh 0.368 g, determine the value for n in the formula.

Interpretation Introduction

Interpretation: The general formula of a xenon fluoride compound is given as XeFn . The value of n is to be calculated.

Concept introduction: The number of atoms of an element in a particular compound (n) can be calculated using the mass of all the atoms of that element present in the given compound and the atomic mass of that element. The formula can be stated as,

n=TotalmassofelementinthegivencompoundAtomicmassoftheelement

To determine: The value of n in XeFn .

Explanation

Given

The mass of 9.03×1020molecules of XeFn is 0.368g .

The mass of 1molecule of XeFn =(0.3689.03×1020)g

The mass of 6.022×1023molecules of XeFn =(0.368×6.022×10239.03×1020)g=245.41g

6.022×1023molecules is equal to one mole of any substance.

Therefore,

The mass of 1mol of XeFn =245.41g

The atomic mass of xenon is 131.3g/mol

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