   # A 0509-g sample of an unknown organic compound containing C, H, and O was burned in air to give 1.316 g of CO 2 and 0.269 g of H 2 O. What is the empirical formula for this compound? (a) CHO (b) C 2 H 2 O (c) C 4 H 4 O (d) CHO 4 ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 4.4, Problem 1RC
Textbook Problem
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## A 0509-g sample of an unknown organic compound containing C, H, and O was burned in air to give 1.316 g of CO2 and 0.269 g of H2O. What is the empirical formula for this compound? (a) CHO (b) C2H2O (c) C4H4O (d) CHO4

Interpretation Introduction

Interpretation:

The empirical formula of given unknown organic compound should be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
•  The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).

### Explanation of Solution

From the given masses the amount of CO2andH2O can be calculated.

Thus, amount of CO2andH2O isolated from the combustion are,

1.316gCO2×1molCO244.010gCO2=0.0299molCO20.269gH2O×1molH2O18.015gH2O=0.01493molH2O

For every mole of CO2 isolated, 1 mol of C must have been present in the styrene compound.

So,

0.0299molCO2×1molCinunknown1molCO2=0.0299molC

For every mole of H2O isolated, 2 mol of H must have been present in the unknown compound.

Therefore,

0.01493molH2O×2molHinunknown1molH2O=0.02986molH

The mass of oxygen in the sample can be determined from the mass of original sample and the masses of carbon and oxygen in the sample as follows,

Massofsample=1.316g=0.3588gC+0

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