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Chapter 9: Problem 124

If you have \(44.6 \mathrm{~g}\) of carbon tetrachloride, how many atoms of chlorine do you have?

Short Answer

Expert verified
In 44.6 g of carbon tetrachloride (\(CCl_4\)), there are approximately \(6.98 \times 10^{23}\) atoms of chlorine.

Step by step solution

01

Find the molar mass of carbon tetrachloride

Carbon tetrachloride has a molecular formula of \(CCl_4\), which consists of 1 carbon atom and 4 chlorine atoms. To find the molar mass of carbon tetrachloride, we need to find the molar mass of carbon and chlorine and then add them according to the molecular formula. The molar mass of carbon (C) is 12.01 g/mol, and the molar mass of chlorine (Cl) is 35.45 g/mol. Molar mass of \(CCl_4 = 1 \times (12.01) + 4 \times (35.45) = 12.01 + 141.8 = 153.81\) g/mol.
02

Calculate the number of moles of carbon tetrachloride

Now that we know the molar mass of carbon tetrachloride, we can find the number of moles present in 44.6 grams of the substance using the formula: Number of moles = \(\frac{\text{mass of substance}}{\text{molar mass}}\) Number of moles of \(CCl_4 = \frac{44.6}{153.81} = 0.29 \) moles.
03

Determine the number of moles of chlorine atoms

In each molecule of carbon tetrachloride, there are 4 chlorine atoms. Thus, the number of moles of chlorine atoms is 4 times the number of moles of carbon tetrachloride. Number of moles of chlorine atoms = \(4 \times 0.29 = 1.16\) moles.
04

Calculate the number of chlorine atoms using Avogadro's number

Finally, we can calculate the number of chlorine atoms using Avogadro's number, which is approximately \(6.022 \times 10^{23}\) particles per mole. Number of chlorine atoms = number of moles of chlorine atoms × Avogadro's number Number of chlorine atoms = \(1.16 \times (6.022 \times 10^{23}) = 6.98 \times 10^{23}\) atoms. Note that the result has been rounded to two significant figures, as there were two significant figures in the original mass of carbon tetrachloride. So, there are approximately \(6.98 \times 10^{23}\) atoms of chlorine in 44.6 grams of carbon tetrachloride.

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Most popular questions from this chapter

The ingredients for making 1 dozen cupcakes are: 5 tablespoons butter 1 cup sugar 2 eggs 2 cups flour 1 cup milk If you have only 5 eggs but plenty of all of the other ingredients: (a) How many cupcakes can you make? (b) How many cups of sugar do you need to make the number of cupcakes calculated in (a)?

Consider the unbalanced chemical equation \(\mathrm{N}_{2} \mathrm{O}_{4}+\mathrm{N}_{2} \mathrm{H}_{4} \rightarrow \mathrm{N}_{2}+\mathrm{H}_{2} \mathrm{O}\) (a) Balance the equation. (b) If \(42.32 \mathrm{~g}\) of \(\mathrm{N}_{2}\) was produced and the reaction yield was \(67.5 \%\), how many grams of \(\mathrm{N}_{2} \mathrm{O}_{4}\) and \(\mathrm{N}_{2} \mathrm{H}_{4}\) were consumed in the reaction?

(a) What is the molar mass of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) ?\) (b) What is the mass of \(1.25\) moles of sucrose? (c) How many sucrose molecules are in \(1.25\) moles? (d) How many hydrogen atoms are in \(1.25\) moles of sucrose? (e) What is the mass in grams of the hydrogen atoms in part (d)?

How many grams of glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) would you need to get \(5.00 \times 10^{30}\) carbon atoms?

Caffeine is made up of \(49.48 \%\) by mass \(C, 5.19 \%\) by mass \(\mathrm{H}, 28.85 \%\) by mass \(\mathrm{N}\), and \(16.48 \%\) by mass \(\mathrm{O}\). If its molar mass is approximately \(194 \mathrm{~g} / \mathrm{mol}\), what is the molecular formula of caffeine?
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