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You are given an unknown gaseous binary compound (that is, a compound consisting of two different elements). When 10.0 g of the compound is burned in excess oxygen, 16.3 g of water is produced. The compound has a density 1.38 times that of oxygen gas at the same conditions of temperature and pressure. Give a possible identity for the unknown compound.

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Chemistry: An Atoms First Approach

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

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 161CP
Textbook Problem
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You are given an unknown gaseous binary compound (that is, a compound consisting of two different elements). When 10.0 g of the compound is burned in excess oxygen, 16.3 g of water is produced. The compound has a density 1.38 times that of oxygen gas at the same conditions of temperature and pressure. Give a possible identity for the unknown compound.

Interpretation Introduction

Interpretation: The possible identity of diatomic compound having a density of 1.38 times of O2 at same temperature and pressure should be identified, if the 10g of compound is producing 16.3g of H2O while burning in oxygen.

Concept introduction:

  • Equation for number of moles are,

Number of moles=MassMolarmass

  • According to ideal gas equation for molar mass in terms of density is,

Molarmass=Density×R×Temperaturepressure

  • Mass of a substance from its number of moles is,

Number of moles×Molecularmass in grams=takenMass

  • Mole ratios between the reactant and products of a reaction are depends upon the coefficients of respective reactant in a balanced chemical equation.

Explanation of Solution

Explanation

To find: the molar mass of given unknown diatomic compound.

The molar mass of given unknown diatomic compound is 44.2g .

The density of unknown diatomic compound is 1.38 times of density of O2.

According to ideal gas equation for molar mass in terms of density is,

Molarmass=Density×R×Temperaturepressure

At constant temperature and pressure,

molarmassdensity

Therefore,

molarmassofgivencompoundmolarmassofO2densityofgivencompounddensity ofO2

The molar mass of O2 is 32 g.

Then, the molar mass of given compound is,

molarmassofgivencompound=1.38×molarmassofO2 =1.38×32=44.2

Hence,

The molar mass of given unknown diatomic compound is 44.2g.

To find: the number of moles of unknown diatomic compound and produced 16.3g of H2O in the given reaction.

The number of moles of unknown diatomic compound is 0.4443mol.

The number of moles of produced H2O is 0.4443mol.

Let’s take the formula for unknown diatomic compound is AxHy(since the compound should have a H-element because it is producing H2O while burning in O2).

The mass of AxHy is given as 10g.

The molar mass of given AxHy is 44.2 g

The mass of H2O is given as 16.3 g.

The molar mass of O2 is 32 g.

Equation for number of moles is,

Number of moles=MassMolarmass

Therefore,

The number of moles of AxHy is,

Number of moles=10g44.2g/mol=0

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Chapter 8 Solutions

Chemistry: An Atoms First Approach
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