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Chapter 7: Problem 33

Calculate the mass of each of the following samples: a. 0.500 \(\mathrm{mol} \mathrm{I}_{2}\) (molar mass of \(\mathrm{I}_{2}=\) 253.80 \(\mathrm{g} / \mathrm{mol} )\) b. 2.82 mol PbS (molar mass of PbS = 239.3 g/mol) c.4 .00 \(\mathrm{mol}\) of \(\mathrm{C}_{4} \mathrm{H}_{10}\) (molar mass of \(\mathrm{C}_{4} \mathrm{H}_{10}=\) 58.14 \(\mathrm{g} / \mathrm{mol} )\)

Short Answer

Expert verified
The masses of the samples are: a. 126.9 g b. 674.5 g c. 232.6 g

Step by step solution

01

Calculate mass of I2

To find the mass of \(0.500 \mathrm{mol} \mathrm{I}_{2}\), multiply 0.500 moles by its molar mass (253.80 \(\mathrm{g} / \mathrm{mol}\)). Using the formula, mass = mol * molar mass, the mass is found to be \(0.500 \mathrm{mol} * 253.80 \mathrm{g} / \mathrm{mol} = 126.9 g\)
02

Calculate mass of PbS

To find the mass of \(2.82 \mathrm{mol}\) PbS, multiply 2.82 moles by its molar mass (239.3 \(\mathrm{g} / \mathrm{mol}\)). Using the formula, mass = mol * molar mass, the mass is found to be \(2.82 \mathrm{mol} * 239.3 \mathrm{g} / \mathrm{mol} = 674. 5g\)
03

Calculate mass of C4H10

To find the mass of \(4.00 \mathrm{mol}\) \( \mathrm{C}_{4} \mathrm{H}_{10}\), multiply 4.00 moles by its molar mass (58.14 \(\mathrm{g} / \mathrm{mol}\)). Using the formula, mass = mol * molar mass, the mass is found to be \(4.00\mathrm{mol} * 58.14\mathrm{g} / \mathrm{mol} = 232.6g\)

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Most popular questions from this chapter

Oleic acid has the empirical formula \(\mathrm{C}_{9} \mathrm{H}_{17} \mathrm{O} .\) If the experimental molar mass is \(282 \mathrm{g} / \mathrm{mol},\) what is the molecular formula of oleic acid?

How many moles of sodium ions are there in a sample of salt water that contains \(4.11 \times 10^{22} \mathrm{Na}^{+}\) ions?

Determine the molecular formula for a compound with the empirical formula \(\mathrm{CoC}_{4} \mathrm{O}_{4}\) and a molar mass of 341.94 \(\mathrm{g} / \mathrm{mol} .\)

Research methods scientists initially used to find Avogadro's number. Then compare these methods with modern methods.

How many moles of magnesium oxide are there in \(2.50 \times 10^{25}\) formula units of MgO?
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