   Chapter 10, Problem 78GQ

Chapter
Section
Textbook Problem

A xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in a pressure-proof container. Assume that xenon gas was added to a 0.25-L container until its pressure reached 0.12 atm at 0.0 °C. Fluorine gas was then added until the total pressure reached 0.72 atm at 0.0 °C. After the reaction was complete, the xenon was consumed completely, and the pressure of the F2 remaining in the container was 0.36 atm at 0.0 °C. What is the empirical formula of the xenon fluoride?

Interpretation Introduction

Interpretation:

The Xenon Fluride compound prepared from (Xe) and (F2) gas, with high temperature and pressure.  In this statement both reactants pressure and temperature are given, using this values the (XeF2) empirical formula should identified.

Concept Introduction:

The empirical formula methods

Empirical formula: This concept given that formula that gives the simplest whole number ratio of atoms in a compound.

1. 1. Start with the number of grams of each element, given in the problem.
2. 2. Convert the mass of each element to moles using the molar mass from the periodic table.
3. 3. Divide each mole value by the smallest number of moles calculated.
4. 4. Round to the nearest whole number.  This is the mole ratio of the elements and is.
Explanation

Let us consider the given values of reactant and product

The xenon fluride is the first element in the formula (Xe), because is has no prefix and nothing to tell us differently, we assume that there is only one if Xe.  Than difluoride have two fluorine atoms.  It refers to the symbol of (F), next we consider the fallowing some empirical formula of XeF2

The Molar mass of XeF2 is =169.2898g/mol

ThecompoundhasXenonflurideformulainHillsystemis(XeF2)ThanelementcompositionofXeF2SingleAtomicweightof(Xe)=131

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