Calculate the mass in grams of each of the following...

Calculate the mass in grams of each of the following samples. a. 1.50 mol of aluminum iodide b. $1.91 \times 10^{-3}$ mol of benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$ c. 4.00 mol of glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ d. $4.56 \times 10^{5}$ mol of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ e. 2.27 $\mathrm{mol}$ of calcium nitrate

Calculate the mass in grams of each of the following samples.
a. 1.50 mol of aluminum iodide
b. $1.91 \times 10^{-3}$ mol of benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$
c. 4.00 mol of glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
d. $4.56 \times 10^{5}$ mol of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
e. 2.27 $\mathrm{mol}$ of calcium nitrate

Key Concepts

Unit Conversion

Unit conversion in this context involves converting moles to grams using the molar mass as a conversion factor. The process is straightforward: multiply the number of moles by the molar mass to obtain the mass in grams. This conversion is essential in quantitative chemistry to relate laboratory measurements to the number of particles involved.

Atomic Mass and Chemical Formula

Atomic mass is the mass of an individual atom, usually expressed in atomic mass units (amu), while a chemical formula shows the types and numbers of atoms present in a molecule. Using the chemical formula, one can determine the molar mass by multiplying the atomic masses of the individual atoms by their respective counts and summing them up.

Mole Concept

The mole is a fundamental unit in chemistry that measures the amount of substance. One mole contains Avogadro's number (approximately 6.022 x 10^23) of particles, be they atoms, molecules, ions, or electrons. This concept allows chemists to translate between the mass of substances and the number of particles involved in chemical reactions.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a given molecular formula. This value is crucial for converting between the amount in moles and the mass in grams.

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