# When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. :math&gt; C ( s ) + O 2 ( g ) → CO 2 ( g ) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. :math&gt; 2C ( s ) + O 2 ( g ) → CO ( g ) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?

### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425

Chapter
Section

### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
Chapter 9, Problem 29QAP
Textbook Problem
145 views

## When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide.:math> C ( s ) + O 2 ( g ) → CO 2 ( g ) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result.:math> 2C ( s ) + O 2 ( g ) → CO ( g ) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?

Interpretation Introduction

Interpretation:

The mass of each product formed from burning of 5.00 g sample of pure carbon under each condition should be calculated.

Concept Introduction:

The incomplete combustion of hydrocarbon results in the formation of carbon monoxide and water. It takes place in limited amount of oxygen. The complete combustion of hydrocarbon or in the presence of excess of oxygen, carbon dioxide and water are formed as products.

### Explanation of Solution

When oxygen is present in excess, the reaction for burning of carbon is represented as follows:

C(s)+O2(g)CO2(g)

From the above reaction, the product formed is carbon dioxide and 1 mol of carbon form 1 mol of carbon dioxide.

To determine the mass of carbon dioxide, first calculate the number of moles of pure carbon in given mass of carbon as follows:

n=mM

The molar mass of carbon is 12 g/mol thus,

n=5.0 g12.0 g/mol=0.417 mol

From the balanced chemical reaction, 1 mol of pure carbon gives 1 mol of carbon dioxide thus, 0.417 mol will give 0.417 mol of carbon dioxide.

Molar mass of carbon dioxide is 44 g/mol, calculate mass of carbon dioxide as follows:

m=n×M

Putting the values,

m=(0

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