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Chapter 2: Problem 55

What is the total number of atoms in (a) 15.8 mol \(\mathrm{Fe}\); (b) \(0.000467 \mathrm{mol} \mathrm{Ag} ;\) (c) \(8.5 \times 10^{-11} \mathrm{mol} \mathrm{Na} ?\)

Short Answer

Expert verified
The total number of atoms are: (a) \(9.51 \times 10^{24}\) atoms Fe, (b) \(2.81 \times 10^{20}\) atoms Ag, and (c) \(5.12 \times 10^{13}\) atoms Na.

Step by step solution

01

Calculate the total number of Fe atoms

Multiply the given number of Fe moles by Avogadro's number to find the total number of Fe atoms. The calculation will be: \(15.8 \, \text{mol Fe} \times 6.022 \times 10^{23} \text{ atoms/mol} = 9.51 \times 10^{24}\, \text{atoms Fe}\).
02

Calculate the total number of Ag atoms

Multiply the given number of Ag moles by Avogadro's number to find the total number of Ag atoms. The calculation will be: \(0.000467 \, \text{mol Ag} \times 6.022 \times 10^{23}\, \text{ atoms/mol} = 2.81 \times 10^{20}\, \text{atoms Ag}\).
03

Calculate the total number of Na atoms

Multiply the given number of Na moles by Avogadro's number to find the total number of Na atoms. The calculation will be: \(8.5 \times 10^{-11} \, \text{mol Na} \times 6.022 \times 10^{23} \, \text{atoms/mol} = 5.12 \times 10^{13}\, \text{atoms Na}\).

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Most popular questions from this chapter

A mass spectrum of germanium displayed peaks at mass numbers \(70,72,73,74,\) and \(76,\) with relative heights of \(20.5,27.4,7.8,36.5,\) and \(7.8,\) respectively. (a) In the manner of Figure \(2-14,\) sketch this mass spectrum. (b) Estimate the weighted-average atomic mass of germanium, and state why this result is only approximately correct.

There are three naturally occurring isotopes of magnesium. Their masses and percent natural abundances are \(23.985042 \mathrm{u}, 78.99 \% ; 24.985837 \mathrm{u}, 10.00 \% ;\) and \(25.982593 \mathrm{u}, 11.01 \% .\) Calculate the weighted-average atomic mass of magnesium.

A 0.406 g sample of magnesium reacts with oxygen, producing \(0.674 \mathrm{g}\) of magnesium oxide as the only product. What mass of oxygen was consumed in the reaction?

For the ion \(^{228} \mathrm{Ra}^{2+}\) with a mass of 228.030 u, determine (a) the numbers of protons, neutrons, and electrons in the ion; (b) the ratio of the mass of this ion to that of an atom of \(^{16} \mathrm{O}\) (refer to page 47 ).

In one experiment, 2.18 g sodium was allowed to react with \(16.12 \mathrm{g}\) chlorine. All the sodium was used up, and 5.54 g sodium chloride (salt) was produced. In a second experiment, 2.10 g chlorine was allowed to react with \(10.00 \mathrm{g}\) sodium. All the chlorine was used up, and 3.46 g sodium chloride was produced.Show that these results are consistent with the law of constant composition.
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