   Chapter 13, Problem 85QAP ### 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
195 views

# Calcium oxide can be used to “scrub" carbon dioxide from air.msp;  CaO ( s ) + CO 2 ( g ) CaCO3 ( s ) at mass of CO 2 could he absorbed by 1 . 25 g of CaO ? What volume would this CO 2 occupy an STP?

Interpretation Introduction

Interpretation:

The mass of CO2 and volume of CO2 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 CaO is 1.25 g

Calculation:

The balanced chemical reaction is as follows:

CaO(s)+CO2(g)CaCO3(s)

From the balanced chemical reaction, 1 mol of CaO reacts with 1 mol of CO2. To calculate the mass of CO2, first calculate the number of moles of both CaO and CO2.

n=mM

Molar mass of CaO is 56.08 g/mol thus,

n=1.25 g56.08 g/mol=0.022 mol

Since, 1 mol of CaO reacts with 1 mol of CO2 thus, 0.022 mol of CaO will react with 0.022 mol of CO2.

From number of moles of gas, mass can be calculated as follows:

m=n×M

Molar mass of CO2 is 44

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