Question

a particular vitamins chemical formula has one cobalt atom. what is the molar mass of the vitamin if it contains 4.34% cobalt?

Explanation:

Step1: Determine the molar mass of cobalt

The molar mass of cobalt (\(Co\)) is \(58.93\ g/mol\).

Step2: Set up the equation for mass percentage

The mass percentage of cobalt in the vitamin is given by the formula \(\text{Mass}\%=\frac{\text{Mass of }Co}{\text{Molar mass of vitamin}}\times100\). Let \(M\) be the molar mass of the vitamin. We know that \(\text{Mass}\% = 4.34\%\) and the mass of \(Co\) in one - mole of the vitamin is \(58.93\ g\) (since there is one \(Co\) atom per molecule of the vitamin). So, \(4.34=\frac{58.93}{M}\times100\).

Step3: Solve for \(M\)

First, rewrite the equation as \(M=\frac{58.93\times100}{4.34}\).

$$M=\frac{5893}{4.34}$$

$$M = 1358\ g/mol$$

Answer:

\(1358\ g/mol\)