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Chapter 9: Problem 9

How many moles of carbon atoms are there in 2 moles of propane?

Short Answer

Expert verified
There are 6 moles of carbon atoms in 2 moles of propane.

Step by step solution

01

Identify the molecular formula of propane

Propane has a molecular formula of C3H8, meaning that it contains 3 carbon atoms and 8 hydrogen atoms in each molecule.
02

Understand the relationship between moles of propane and moles of carbon atoms

As there are 3 carbon atoms in each molecule of propane, it means that there are 3 times as many moles of carbon atoms as there are moles of propane.
03

Calculate the moles of carbon atoms in 2 moles of propane

Given we have 2 moles of propane, we now multiply the number of moles of propane by the number of carbon atoms in each molecule to find the moles of carbon atoms: Moles of carbon atoms = 2 moles of propane × 3 carbon atoms/mole of propane Moles of carbon atoms = \( 2 \times 3 \)
04

Find the result

Moles of carbon atoms = 6 There are 6 moles of carbon atoms in 2 moles of propane.

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Most popular questions from this chapter

The flavoring agent vanillin contains carbon, hydrogen, and possibly oxygen. When \(0.450 \mathrm{~g}\) of vanillin is subjected to combustion analysis, the results are \(63.08 \% \mathrm{C}\) and \(5.30 \% \mathrm{H}\). If the molar mass is approximately \(152 \mathrm{~g} / \mathrm{mol}\), what is the molecular formula of vanillin?

A gaseous mixture containing \(10.079 \mathrm{~g}\) of \(\mathrm{H}_{2}\) and \(7.00\) moles of \(\mathrm{Br}_{2}\) react to form HBr. (a) Write a balanced chemical equation for this reaction. (b) Which reactant is limiting? (c) What is the theoretical yield for this reaction in moles? (d) What is the theoretical yield for this reaction in grams? (e) How many moles of excess reactant are left over at the end of the reaction? (f) How many grams of excess reactant are left over at the end of the reaction?

Consider the unbalanced chemical equation \(\mathrm{Cl}_{2} \mathrm{O}_{7}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{HClO}_{4}\) The reaction is carried out at \(82.0 \%\) yield and gives \(52.8 \mathrm{~g}\) of \(\mathrm{HClO}_{4}\) (a) What is the theoretical yield of \(\mathrm{HClO}_{4}\) ? (b) How many grams of \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) and \(\mathrm{H}_{2} \mathrm{O}\) were consumed in the reaction?

Consider the unbalanced chemical equation \(\mathrm{As}_{4} \mathrm{~S}_{6}+\mathrm{O}_{2} \rightarrow \mathrm{As}_{4} \mathrm{O}_{6}+\mathrm{SO}_{2}\) (a) How many grams of \(\mathrm{O}_{2}\) are needed to react completely with \(58.9 \mathrm{~g}\) of \(\mathrm{As}_{4} \mathrm{~S}_{6}\) ? (b) If \(41.2 \mathrm{~g}\) of \(\mathrm{SO}_{2}\) is produced, what is the percent yield for the reaction?

How many grams of sulfur hexafluoride would you need to have \(5.25 \times 10^{24}\) fluorine atoms?
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