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Number of molecules in 3.5g H?O, 56.1g N?, 89g CCl?, 19g C?H??O?
Chapter 6, Problem 53P(choose chapter or problem)
How many molecules are in each sample?
(a) 3.5 g \(\mathrm{H}_{2} \mathrm{O}\)
(b) 56.1 g \(\mathrm{N}_{2}\)
(c) 89 g \(\mathrm{CCl}_{4}\)
(d) 19 g \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)
Questions & Answers
QUESTION:
How many molecules are in each sample?
(a) 3.5 g \(\mathrm{H}_{2} \mathrm{O}\)
(b) 56.1 g \(\mathrm{N}_{2}\)
(c) 89 g \(\mathrm{CCl}_{4}\)
(d) 19 g \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)
ANSWER:Step 1 of 4
To determine the number of molecules in each sample, we use the concept of moles. One mole of any substance contains Avogadro's number, approximately \(6.022 \times 10^{23}\), of its elementary entities, which can be atoms, molecules, ions, etc.
We first convert the mass of the substance to moles using the molar mass, then we multiply it by Avogadro's number.
(a) we have 3.5 g of water \(\mathrm{H}_{2} \mathrm{O}\)
Calculating the molar mass of of \mathrm{H}_{2} \mathrm{O}\)
\(\begin{aligned} \text { molar mass } & =1 \times(16.00)+2 \times(1.008) \\ & =16+2.016 \\ & =18.02 \mathrm{~g} / \mathrm{mol} \end{aligned}\)
Calculating the number of molecules in 3.5 g of \(\mathrm{H}_{2} \mathrm{O}\)
\(\left(\frac{3.5}{18.02}\right) \times 6.022 \times 10^{23} = 1.17 \times 10^{23}\)
Therefore, 3.5 g of of \(\mathrm{H}_{2} \mathrm{O}\) contains \(1.17 \times 10^{23}\) molecules of \(\mathrm{H}_{2} \mathrm{O}\).
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Number of molecules in 3.5g H?O, 56.1g N?, 89g CCl?, 19g C?H??O?
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This video shows how to determine the number of molecules in a given sample by utilizing the concept of moles, Avogadro's number (6.022 x 10²³), and the molar mass of the substance. It provides step-by-step calculations for different substances, converting mass to the number of molecules and highlighting the versatile application of this approach.