Calculate the number of moles of carbon atoms present in...

Calculate the number of moles of carbon atoms present in each of the following samples. a. 1.271 g of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ b. 3.982 $\mathrm{g}$ of $1,4$ -dichlorobenzene, $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$ c. 0.4438 $\mathrm{g}$ of carbon suboxide, $\mathrm{C}_{3} \mathrm{O}_{2}$ d. 2.910 $\mathrm{g}$ of methylene chloride, $\mathrm{CH}_{2} \mathrm{Cl}_{2}$

Calculate the number of moles of carbon atoms present in each of the following samples.
a. 1.271 g of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
b. 3.982 $\mathrm{g}$ of $1,4$ -dichlorobenzene, $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$
c. 0.4438 $\mathrm{g}$ of carbon suboxide, $\mathrm{C}_{3} \mathrm{O}_{2}$
d. 2.910 $\mathrm{g}$ of methylene chloride, $\mathrm{CH}_{2} \mathrm{Cl}_{2}$

Key Concepts

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the use of mole ratios derived from chemical formulas to convert between amounts of different substances, such as determining the number of moles of a specific element in a given mass of a compound.

Chemical Formula Interpretation

Interpreting chemical formulas involves understanding the composition of a compound through the symbols and subscripts that indicate the number and types of atoms present. This skill is necessary to determine the contribution of individual elements within a compound, such as counting the number of carbon atoms per molecule.

Molar Mass Calculation

Molar mass is the mass of one mole of a substance and is calculated by summing the atomic masses of all atoms in a molecule as given by its chemical formula. It is crucial for converting between the mass of a substance and the number of moles, which is a common requirement in quantitative chemical analysis.

Mole Concept

The mole is a fundamental unit in chemistry that represents a specific quantity of particles, usually atoms or molecules, equivalent to Avogadro's number (approximately 6.022 x 10^23). It serves as a bridge between the atomic scale and the macroscopic measurements in the lab, allowing chemists to count particles by weighing them.

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