Question

The compound known as diethyl ether, commonly referred to as ether, contains carbon, hydrogen, and oxygen. A 3.626 g sample of ether was combusted in an oxygen rich environment to produce 8.612 g of CO2(g) and 4.406 g of H2O(g). Insert subscripts to complete the empirical formula of ether.

Answer 1

`C_4H_(10)O`

Step-by-step explanation:

Hello,

In this case, the first step is to compute the moles of carbon in the sample that are contained in CO2 only at the products as shown below:

`n_C=8.612gCO_2*(1molCO_2)/(44gCO_2) *(1molC)/(1molCO_2) =0.196molC`

Next the moles of hydrogen contained in the H2O only:

`n_H=4.406gH_2O*(1molH_2O)/(18gH_2O) *(2molH)/(1molH_2O) =0.490molH`

Now, we compute the mass of oxygen in the sample, by subtracting mass of both carbon and hydrogen from the 3.626 g of sample:

`m_O=3.626g-0.196molC*(12gC)/(1molC)-0.490molH*(1gH)/(1molH) =0.784gO`

And the moles:

`n_O=0.784gO*(1molO)/(16gO) =0.049molO`

Now, the mole ratios by considering the moles of oxygen as the smallest:

`C=(0.196mol)/(0.049mol)= 4\\\\H=(0.49mol)/(0.049mol)=10\\\\O=(0.049mol)/(0.049mol)=1`

Thus, empirical formula is:

`C_4H_(10)O`

Regards.