Concept explainers
(a)
Interpretation:
The number of molecules present in the samples needs to be predicted.
Concept Introduction:
Mole is the amount of the substance that contains the same number of particles or atoms or molecules. Molar mass is defined as an average
(a)
Answer to Problem 26A
Number of molecules of CO in 6.37 mol = 3.836 ×1022 molecules
Explanation of Solution
Number of molecules in 6.37 mol of carbon monoxide
Number of carbon monoxide molecules = Number of moles ×
= 6.37 mol × (6.022140857 × 1023 molecules / mol)
= 38.361 × 1023 molecules
= 3.836 ×1022 molecules
(b)
Interpretation:
The number of molecules present in the samples needs to be predicted.
Concept Introduction:
Mole is the amount of the substance that contains the same number of particles or atoms or molecules. Molar mass is defined as an average mass of atoms present in the chemical formula. It is the sum of the atomic masses of all the atoms present in the chemical formula of any compound.
(b)
Answer to Problem 26A
Number of molecules of CO in 6.37 g = 1.37 × 1023 molecules
Explanation of Solution
Number of molecules in 6.37 g carbon monoxide
Molecular formula = CO
Molecular mass = 28.01 g/ mol
Given,
Mass of CO = 6.37g
The calculation of moles is shown below:
Number of CO molecules = Number of moles × Avogadro number
= 0.227418779 mol × (6.022140857 × 1023 molecules / mol)
= 1.37 ×1023 molecules
(c)
Interpretation:
The number of molecules present in the samples needs to be predicted.
Concept Introduction:
Mole is the amount of the substance that contains the same number of particles or atoms or molecules. Molar mass is defined as an average mass of atoms present in the chemical formula. It is the sum of the atomic masses of all the atoms present in the chemical formula of any compound.
(c)
Answer to Problem 26A
Number of molecules of H2O in 2.62 ×10-6 g = 8.76× 1016 molecules
Explanation of Solution
Number of molecules in 2.62×10-6 g water
Molecular formula = H2O
Molecular mass = 18g/ mol
Given,
Mass of H2O = 2.62×10-6 g
The calculation of moles is shown below:
Number of H2O molecules = Number of moles × Avogadro number
= 1.4555 ×10-7 mol × (6.022140857 × 1023 molecules / mol)
= 8.76 ×1016 molecules
(d)
Interpretation:
The number of molecules present in the samples needs to be predicted.
Concept Introduction:
Mole is the amount of the substance that contains the same number of particles or atoms or molecules. Molar mass is defined as an average mass of atoms present in the chemical formula. It is the sum of the atomic masses of all the atoms present in the chemical formula of any compound.
(d)
Answer to Problem 26A
Number of molecules of H2O in 2.62× 10-6 mol = 1.58 ×1018 molecules
Explanation of Solution
Number of molecules in 2.62 × 10-6 mol of water
Number of water molecules = Number of moles × Avogadro number
= 2.62 × 10-6 mol × (6.022140857 × 1023 molecules / mol)
= 15.78 × 1017 molecules
= 1.58 ×1018 molecules
(e)
Interpretation:
The number of molecules present in the samples needs to be predicted.
Concept Introduction:
Mole is the amount of the substance that contains the same number of particles or atoms or molecules. Molar mass is defined as an average mass of atoms present in the chemical formula. It is the sum of the atomic masses of all the atoms present in the chemical formula of any compound.
(e)
Answer to Problem 26A
Number of molecules of C6H6 in 5.23 g = 4.029× 1022 molecules
Explanation of Solution
Number of molecules in 5.23 g benzene
Molecular formula = C6H6
Molecular mass = 78.11 g/ mol
Given,
Mass of C6H6= 5.23 g
The calculation of moles is shown below:
Number of C6H6 molecules = Number of moles × Avogadro number
= 0.0669 mol × (6.022140857 × 1023 molecules / mol)
= 4.029 ×1022 molecules
Chapter 6 Solutions
World of Chemistry, 3rd edition
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