# Question 201b5

Aug 1, 2017

$0.538$ $\text{g}$ $\text{^13"C}$

#### Explanation:

We're asked to find the number of moles of $\text{^13"C}$ that has a mass of $7.00$ $\text{g}$.

Carbon-13 is merely an isotope of carbon, and its isotopic mass is $13.003$ $\text{amu}$ (from a source), which means its molar mass is $13.003$ $\text{g/mol}$.

Thus, we use this molar mass when performing our conversion from mass to moles:

7.00cancel("g"color(white)(l)""^13"C")((1color(white)(l)"mol"color(white)(l)""^13"C")/(13.003cancel("g"color(white)(l)""^13"C"))) = color(red)(ul(0.538color(white)(l)"mol"color(white)(l)""^13"C"#