   # An element X forms both a dichloride (XCl 2 ) and a tetrachloride (XC 4 ). Treatment of 10.00 g XCl 2 with excess chlorine forms 12.55 g XCl 4 . Calculate the atomic mass of X, and identify X. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 5, Problem 173CP
Textbook Problem
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## An element X forms both a dichloride (XCl2) and a tetrachloride (XC4). Treatment of 10.00 g XCl2 with excess chlorine forms 12.55 g XCl4. Calculate the atomic mass of X, and identify X.

Interpretation Introduction

Interpretation: It is given that, when element X reacts with excess of chlorine then both XCl2 and XCl4 is formed. This element X is to be identified and its atomic mass is to be calculated.

Concept introduction: The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

To determine: The name of element X and its atomic mass.

### Explanation of Solution

Given

The mass of XCl2 is 10.0g .

The mass of XCl4 is 12.55g .

The atomic mass of chlorine (Cl) is 35.45g/mol .

The reaction of XCl2 with XCl4 is,

XCl2+excessCl2XCl4

Molar mass is the sum of atomic mass of individual atoms. The molar mass of XCl2 is,

A+2(35.45g/mol)

Where,

• A is atomic mass of element X

It is clear from the given reaction that one mole of reactant XCl2 should give one mole of product XCl4 .

Formula

The mass of compound is calculated by using the formula,

Numberofmoles=MassofcompoundMolarmass

Since, number of moles of XCl2 and XCl4 is same, therefore, from above equation,

MassofXCl2MolarmassofXCl2=MassofXCl4MolarmassofXCl4

Substitute the values of mass and atomic mass of XCl2 , XCl4 in above equation

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