Question

The density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 18.2 g of CO2 according to the following chemical equation?

C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

Answer 1

Answer: 12.1 ml of ethanol is needed

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of} CO_2=(18.2g)/(44g/mol)=0.414moles`

`C_2H_5OH(l)+3O_2(g)\rightarrow 2CO_2(g)+3H_2O(l)`

According to stoichiometry :

2 moles of
`CO_2` is produced by = 1 mole of
`C_2H_5OH`

Thus 0.414 moles of
`CO_2` is produced by=
`(1)/(2)* 0.414=0.207moles` of
`C_2H_5OH`

Mass of
`C_2H_5OH=moles* {\text {Molar mass}}=0.207moles* 46.07g/mol=9.54g`

Volume of ethanol =
`\frac{\text {Mass of ethanol}}{\text {density of ethanol}}=(9.54g)/(0.789g/ml)=12.1ml`

12.1 ml of ethanol is needed to produce 18.2 g of
`CO_2`