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Chapter 9: Problem 6

Suppose you have \(120.11 \mathrm{~g}\) of carbon atoms. (a) How many moles of carbon atoms do you have? (b) How many carbon atoms do you have?

Short Answer

Expert verified
(a) You have 10.00 moles of carbon atoms. (b) You have \(6.022\times10^{24}\) carbon atoms.

Step by step solution

01

Recall the molar mass of carbon and Avogadro's number

The molar mass of carbon (C) is 12.01 g/mol. Avogadro's number is the number of atoms or molecules in one mole of any substance, and it is approximately equal to \(6.022\times10^{23}\) particles/mol.
02

Calculate the number of moles of carbon atoms

Given the mass of carbon atoms (120.11 g), we can calculate the number of moles by dividing the mass by the molar mass of carbon: Number of moles of carbon = \(\frac{\text{mass of carbon atoms}}{\text{molar mass of carbon}} = \frac{120.11 \, \text{g}}{12.01 \, \text{g/mol}} \)
03

Calculate the number of moles of carbon atoms

Now divide the mass of carbon atoms by the molar mass of carbon: Number of moles of carbon = \(\frac{120.11 \, \text{g}}{12.01 \, \text{g/mol}} = 10.00 \, \text{mol} \) So, we have 10.00 moles of carbon atoms.
04

Calculate the number of carbon atoms

Now that we have the number of moles of carbon atoms, we can calculate the total number of carbon atoms using Avogadro's number: Number of carbon atoms = Number of moles of carbon × Avogadro's number = \(10.00 \, \text{mol} \times 6.022\times10^{23} \, \text{particles/mol}\)
05

Calculate the number of carbon atoms

Now multiply the number of moles by Avogadro's number: Number of carbon atoms = \(10.00 \, \text{mol} \times 6.022\times10^{23} \, \text{particles/mol} = 6.022\times10^{24} \, \text{carbon atoms}\) So, we have \(6.022\times10^{24}\) carbon atoms.

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Most popular questions from this chapter

Consider the following unbalanced chemical equation: \(\mathrm{P}+\mathrm{O}_{2} \rightarrow \mathrm{P}_{2} \mathrm{O}_{5}\) (a) How many grams of phosphorus (P) are required to react completely with \(20.0 \mathrm{~g}\) of \(\mathrm{O}_{2} ?\) (b) What is the theoretical yield in grams if you combine the amounts of reactants in part (a)?

Copper reacts with nitric acid as shown in the balanced chemical equation \(3 \mathrm{Cu}+8 \mathrm{HNO}_{3} \rightarrow 3 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}+2 \mathrm{NO}+4 \mathrm{H}_{2} \mathrm{O}\) If you react \(25.0 \mathrm{~g}\) of copper with an excess of nitric acid and produce \(7.24 \mathrm{~g}\) of \(\mathrm{NO}\), what is the percent yield for the reaction?

Ethanol, the alcohol in beer and wine, has the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} .\) Calculate the mass percent of each element in ethanol.

The compound \(\mathrm{P}_{4} \mathrm{O}_{10}\) has an empirical formula of \(\mathrm{P}_{2} \mathrm{O}_{5} .\) By what factor will the percent by mass composition differ for each element between these two formulas? Explain your answer.

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