   Chapter 13, Problem 101QAP ### Introductory Chemistry: A Foundati...

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

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem

# uring the making of steel, iron(II) oxide is reduced to metallic iron by treatment with carbon monoxide gas.msp;  FeO ( s ) + CO ( g )   Fe ( s ) + CO 2 ( g ) ppose 1 . 45 kg of Fe reacts. What volume of CD(g) is required, and what volume of CO 2 ( g ) is produced, each measured at STP?

Interpretation Introduction

Interpretation:

The volume of CO gas required and CO2 gas produced at STP should be calculated.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

The value of Universal gas constant can be taken as 0.082 L atm K1 mol1.

Mass of gas can be calculated from number of moles and molar mass as follows:

m=n×M

Here, n is number of moles, m is mass and M is molar mass.

Explanation

Given Information:

The mass of Fe is 1.45 kg.

Calculation:

The balanced chemical reaction is as follows:

FeO(s)+CO(g)Fe(s)+CO2(g)

To calculate the volume of CO and CO2 gas number of moles of Fe, CO and CO2 should be calculated.

n=mM

Molar mass of Fe is 55.845 g/mol thus,

n=(1.45 kg)(103 g1 kg)(55.845 g/mol)=25.96 mol

From the balanced chemical reaction, 1 mole of FeO reacts with 1 mol of CO to produced 1 mol of Fe (s) and 1 mol of CO2 thus, number of moles of CO and CO2 will be 25

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