Question

How many grams of CO2; will be produced if 13.56 moles of O2, are used to completion? (C2H4 + 3O2=2 CO2, + 2 H2O)

Answer 1

397.8 g of CO2.

Step-by-step explanation:

First, let's write the chemical equation:

`C_2H_4+3O_2\rightarrow2CO_2+2H_2O.`

We want to find the grams of CO2 produced by 13.56 moles of O2, so we can find how many moles of CO2 are being produced, so we can do a rule of three based on this logic: you can see that we have 3 moles of O2 reacted producing 2 moles of CO2, so how many moles would we obtain from 13.56 moles of O2?:

`\begin{gathered} 3\text{ moles O}_2\rightarrow2\text{ moles CO}_2 \\ 13.56\text{ moles O}_2\rightarrow?\text{ moles CO}_2 \end{gathered}`

The calculation would be:

`13.56\text{ moles O}_2\cdot\frac{2\text{ moles CO}_2}{3\text{ moles O}_2}=9.04\text{ moles CO}_2.`

The final step is to convert from 9.04 moles of CO2 to grams using its molar mass which is 44 g/mol (you can calculate the molar mass of a compound using the periodic table). The conversion would look like this:

`9.04\text{ moles CO}_2\cdot\frac{44\text{ g CO}_2}{1\text{ mol CO}_2}=397.8\text{ g CO}_2.`

We will produce 397.8 g of CO2.