General Chemistry
General Chemistry
4th Edition
ISBN: 9781891389603
Author: Donald A. McQuarrie, Peter A. Rock, Ethan B. Gallogly
Publisher: University Science Books
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Chapter 11, Problem 11.1P

(a)

Interpretation Introduction

Interpretation:

The number of moles in 52 g calcium carbonate has to be determined.

Concept Introduction:

Mole is S.I. unit. The number of moles is calculated as ratio of mass of compound to molar mass of compound.

Molar mass is sum of the total mass in grams of all atoms that make up mole of particular molecule that is mass of 1 mole of compound. The S.I unit is g/mol.

The expression to relate number of moles, mass and molar mass of compound is as follows:

  Number of moles=mass of the compoundmolar mass of the compound

(a)

Expert Solution
Check Mark

Answer to Problem 11.1P

The number of moles in 52 g calcium carbonate is 0.51954 mol.

Explanation of Solution

The formula to calculate number of moles of calcium carbonate is as follows:

  Number of moles of CaCO3=Given mass of CaCO3molar mass of CaCO3        (1)

Substitute 52 g for given mass of CaCO3 and 100.0869 g/mol for molar mass of CaCO3 in equation (1).

  number of moles of CaCO3=52 g100.0869 g/mol=0.51954 mol

(b)

Interpretation Introduction

Interpretation:

The number of moles in ethanol has to be determined

Concept Introduction:

Density is characteristic property of a substance. It is defined as mass per unit volume. It is represented by ρ.

The formula to calculate the density is as follows:

  Density(ρ)=Mass(M)Volume(V)

(b)

Expert Solution
Check Mark

Answer to Problem 11.1P

The number of moles in ethanol is 4.1241 mol.

Explanation of Solution

The formula to calculate the density is as follows:

  Density(ρ)=Mass(M)Volume(V)        (2)

Rearrange equation (2) to calculate the mass of solution.

  Mass(ethanol)=(density)(volume)

Substitute 250 mL for volume of ethanol and 0.76 g/mL for density of ethanol in equation (2).

    Mass(ethanol)=(0.76 g/mL)(250 mL)=190 g

The formula to calculate number of moles of ethanol is as follows:

  Number of moles of ethanol=Given mass of ethanolmolar mass of ethanol        (3)

Substitute 190 g for given mass of ethanol and 46.07 g/mol for molar mass of ethanol in equation (3).

  number of moles of ethanol=190 g46.07 g/mol=4.1241 mol

(c)

Interpretation Introduction

Interpretation:

The number of moles in 28.1 g carbon dioxide has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Expert Solution
Check Mark

Answer to Problem 11.1P

The number of moles in 28.1 g carbon dioxide is 0.63849 mol.

Explanation of Solution

The formula to calculate number of moles of carbon dioxide is as follows:

  Number of moles of carbon dioxide=Given mass of carbon dioxidemolar mass of carbon dioxide        (4)

Substitute 28.1 g for given mass of carbon dioxide and 44.01 g/mol for molar mass of carbon dioxide in equation (4).

  number of moles of carbon dioxide=28.1 g44.01 g/mol=0.63849 mol

(d)

Interpretation Introduction

Interpretation:

The number of moles in 5.5×1022 molecules of sulfur hexafluoride gas has to be determined.

Concept Introduction:

One mole of any substance contains 6.022×1023 formula units. This number is called Avogadro’s number.

The expression is as follows:

    1 mole=6.022×1023 molecules

(d)

Expert Solution
Check Mark

Answer to Problem 11.1P

The number of moles in 5.55×1022 molecules of sulfur hexafluoride gas is 0.09216 mol.

Explanation of Solution

The number of molecules of sulfur hexafluoride gas is 5.55×1022 molecules.

The formula to calculate number of moles is as follows:

  Number of moles=(number of molecules)(1 mol6.022×1023 molecules)

Substitute 5.55×1022 molecules for number of molecules.

  Number of moles=(5.55×1022 molecules)(1 mol6.022×1023 molecules)=0.09216 mol

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Chapter 11 Solutions

General Chemistry

Ch. 11 - Prob. 11.11PCh. 11 - Prob. 11.12PCh. 11 - Prob. 11.13PCh. 11 - Prob. 11.14PCh. 11 - Prob. 11.15PCh. 11 - Prob. 11.16PCh. 11 - Prob. 11.17PCh. 11 - Prob. 11.18PCh. 11 - Prob. 11.19PCh. 11 - Prob. 11.20PCh. 11 - Prob. 11.21PCh. 11 - Prob. 11.22PCh. 11 - Prob. 11.23PCh. 11 - Prob. 11.24PCh. 11 - Prob. 11.25PCh. 11 - Prob. 11.26PCh. 11 - Prob. 11.27PCh. 11 - Prob. 11.28PCh. 11 - Prob. 11.29PCh. 11 - Prob. 11.30PCh. 11 - Prob. 11.31PCh. 11 - Prob. 11.32PCh. 11 - Prob. 11.33PCh. 11 - Prob. 11.34PCh. 11 - Prob. 11.35PCh. 11 - Prob. 11.36PCh. 11 - Prob. 11.37PCh. 11 - Prob. 11.38PCh. 11 - Prob. 11.39PCh. 11 - Prob. 11.40PCh. 11 - Prob. 11.41PCh. 11 - Prob. 11.42PCh. 11 - Prob. 11.43PCh. 11 - Prob. 11.44PCh. 11 - Prob. 11.45PCh. 11 - Prob. 11.46PCh. 11 - Prob. 11.47PCh. 11 - Prob. 11.48PCh. 11 - Prob. 11.49PCh. 11 - Prob. 11.50PCh. 11 - Prob. 11.51PCh. 11 - Prob. 11.52PCh. 11 - Prob. 11.53PCh. 11 - Prob. 11.54PCh. 11 - Prob. 11.55PCh. 11 - Prob. 11.56PCh. 11 - Prob. 11.57PCh. 11 - Prob. 11.58PCh. 11 - Prob. 11.59PCh. 11 - Prob. 11.60PCh. 11 - Prob. 11.61PCh. 11 - Prob. 11.62PCh. 11 - Prob. 11.63PCh. 11 - Prob. 11.64PCh. 11 - Prob. 11.65PCh. 11 - Prob. 11.66PCh. 11 - Prob. 11.67PCh. 11 - Prob. 11.68PCh. 11 - Prob. 11.69PCh. 11 - Prob. 11.70PCh. 11 - Prob. 11.71PCh. 11 - Prob. 11.72PCh. 11 - Prob. 11.73PCh. 11 - Prob. 11.74PCh. 11 - Prob. 11.75PCh. 11 - Prob. 11.76PCh. 11 - Prob. 11.77PCh. 11 - Prob. 11.78PCh. 11 - Prob. 11.79PCh. 11 - Prob. 11.80PCh. 11 - Prob. 11.81PCh. 11 - Prob. 11.82PCh. 11 - Prob. 11.83PCh. 11 - Prob. 11.84PCh. 11 - Prob. 11.85PCh. 11 - Prob. 11.86PCh. 11 - Prob. 11.87PCh. 11 - Prob. 11.88PCh. 11 - Prob. 11.89PCh. 11 - Prob. 11.90PCh. 11 - Prob. 11.91PCh. 11 - Prob. 11.92PCh. 11 - Prob. 11.93P
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Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY