   Chapter 15, Problem 32CR ### 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
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# When calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?

Interpretation Introduction

Interpretation:

The volume of CO2 gas produced by heating 1.25g of CaCO3 is to be calculated.

Concept Introduction:

Avogadro’s hypothesis states that at standard temperature and pressure one mole of an ideal gas occupies 22.4L volume. The volume of a gas at STP is given as:

V=Vmn

Where,

• Vm is the molar volume of an ideal gas with value 22.4Lmol1.
• n is the number of moles of an ideal gas.
Explanation

The molar mass of CaCO3 is 100.087gmol1.

The mass of CaCO3 is 1.25g.

The number of moles of substance is given as:

n=mMm

Where,

• m represents the mass of the substance.
• Mm represents the molar mass of the substance.

Substitute the value of the mass and molar mass of CaCO3 in above equation.

n=1.25g100.087gmol1=0.0125mol

The number of moles of CaCO3 reacted is 0.0466mol.

The given reaction is represented as:

CaCO3sCaOs+CO2g

One mole of CaCO3 produces one mole of CO2 gas after heating

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