Based on your answer in Part A, calculate the number of atoms in this amount of ^{13}C?

Express your answer numerically in atoms of carbon.

The *mole* (abbreviated mol) is a counting unit used to simplify calculations that would otherwise involve very large numbers. The mole is equivalent to the number of carbon atoms in exactly 12 g of isotopically pure ^{12}C, or 6.02 × 10^{23}. This number is known as *Avogadro's number* in honor of Amedeo Avogadro. Avogadro's number can be used as a conversion factor between moles and atoms as shown here:

$\frac{\mathbf{6}\mathbf{.}\mathbf{02}\mathbf{}\mathbf{\times}\mathbf{}{\mathbf{10}}^{\mathbf{23}}\mathbf{}\mathbf{atoms}\mathbf{}}{\mathbf{1}\mathbf{}\mathbf{mole}\mathbf{}\mathbf{of}\mathbf{}\mathbf{atoms}\mathbf{}}$

The *molar mass *of a substance is the mass of one mole of a substance and is written in units of grams per mole. The molar mass of an atom is equivalent to its atomic mass whereas the molar mass of a substance is equivalent to its formula weight.

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