   Chapter 3, Problem 5PS

Chapter
Section
Textbook Problem

Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams of oxygen were required in this reaction?

Interpretation Introduction

Interpretation:

The grams of oxygen required for given reaction should be calculated.

Concept Introduction:

The number of moles can be calculated as follows,

Moles = MassMolar mass

Explanation

The equation is given below,

2 moles of carbon monoxide is reacts with one mole of oxygen which gives the two moles of carbon dioxide.

One gram of carbon monoxide yields 1.57g of carbon dioxide. Therefore,

Number of moles of carbon monoxide,

Number of moles = MassMolar massNumber of moles = 1g28Number of moles = 0.035 moles

Number of moles of carbon monoxide,

Number of moles = MassMolar massNumber of moles = 1

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts 