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Chapter 3: Problem 61

What amount (moles) is represented by each of these samples? a. \(150.0 \mathrm{~g} \mathrm{Fe}_{2} \mathrm{O}_{3}\) b. \(10.0 \mathrm{mg} \mathrm{NO}_{2}\) c. \(1.5 \times 10^{16}\) molecules of \(\mathrm{BF}_{3}\)

Short Answer

Expert verified
a. \(0.939 \mathrm{~mol} \mathrm{Fe}_{2} \mathrm{O}_{3}\) b. \(2.17 \times 10^{-4} \mathrm{~mol} \mathrm{NO}_{2}\) c. \(2.49 \times 10^{-8} \mathrm{~mol} \mathrm{BF}_{3}\)

Step by step solution

01

a. Calculate the moles of Fe鈧侽鈧�.

To calculate the moles of Fe鈧侽鈧�, use the formula: moles = mass / molar mass First, find the molar mass of Fe鈧侽鈧�: Fe = 55.85 g/mol (for 2 Fe atoms = 2 x 55.85 g/mol) O = 16.00 g/mol (for 3 O atoms = 3 x 16.00 g/mol) Molar mass of Fe鈧侽鈧� = 2(55.85 g/mol) + 3(16.00 g/mol) = 159.7 g/mol Now, determine the moles of Fe鈧侽鈧�: moles = 150.0 g / 159.7 g/mol = 0.939 mol
02

b. Calculate the moles of NO鈧�.

To calculate the moles of NO鈧�, use the formula: moles = mass / molar mass First, convert the mass of NO鈧� from mg to g: 10.0 mg = 0.010 g Now, find the molar mass of NO鈧�: N = 14.01 g/mol O = 16.00 g/mol (for 2 O atoms = 2 x 16.00 g/mol) Molar mass of NO鈧� = 14.01 g/mol + 2(16.00 g/mol) = 46.01 g/mol Determine the moles of NO鈧�: moles = 0.010 g / 46.01 g/mol 鈮� 2.17 x 10^{-4} mol
03

c. Calculate the moles of BF鈧�.

To calculate the moles of BF鈧�, use Avogadro's number to convert the given number of molecules to moles: number of moles = number of molecules / Avogadro's number number of moles = (1.5 x 10^16 molecules) / (6.022 x 10^23 molecules/mol) 鈮� 2.49 x 10^{-8} mol

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Most popular questions from this chapter

A compound contains \(47.08 \%\) carbon, \(6.59 \%\) hydrogen, and \(46.33 \%\) chlorine by mass; the molar mass of the compound is \(153 \mathrm{~g} / \mathrm{mol} .\) What are the empirical and molecular formulas of the compound?

A given sample of a xenon fluoride compound contains molecules of the type \(\mathrm{XeF}_{n}\), where \(n\) is some whole number. Given that \(9.03 \times 10^{20}\) molecules of \(\mathrm{XeF}_{n}\) weigh \(0.368 \mathrm{~g}\), determine the value for \(n\) in the formula.

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Express the composition of each of the following compounds as the mass percents of its elements. a. formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\) b. glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) c. acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

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