Questions: Question 40 1 pts An estrogen compound with the empirical formula C12H17O2 has a molecular mass of 386.6 g / mol. What is the value of n necessary to find the molecular formula? 2 0.2 20 1 none of the above

Question 40
1 pts

An estrogen compound with the empirical formula C12H17O2 has a molecular mass of 386.6 g / mol. What is the value of n necessary to find the molecular formula?
2
0.2
20
1
none of the above

Transcript text: Question 40 1 pts An estrogen compound with the empirical formula $\mathrm{C}_{12} \mathrm{H}_{17} \mathrm{O}_{2}$ has a molecular mass of $386.6 \mathrm{~g} / \mathrm{mol}$. What is the value of n necessary to find the molecular formula? 2 0.2 20 1 none of the above

Solution

Solution Steps

Step 1: Calculate the Empirical Formula Mass

First, we need to calculate the empirical formula mass of the compound $\mathrm{C}_{12} \mathrm{H}_{17} \mathrm{O}_{2}$.

Carbon (C): $12 \text{ atoms} \times 12.01 \text{ g/mol} = 144.12 \text{ g/mol}$
Hydrogen (H): $17 \text{ atoms} \times 1.008 \text{ g/mol} = 17.136 \text{ g/mol}$
Oxygen (O): $2 \text{ atoms} \times 16.00 \text{ g/mol} = 32.00 \text{ g/mol}$

Adding these together gives the empirical formula mass: \[ 144.12 + 17.136 + 32.00 = 193.256 \text{ g/mol} \]

Step 2: Determine the Value of $ n $

The molecular mass of the compound is given as $386.6 \text{ g/mol}$. To find the value of $ n $, we divide the molecular mass by the empirical formula mass: \[ n = \frac{386.6 \text{ g/mol}}{193.256 \text{ g/mol}} \approx 2.000 \]