Question

HELP FOR FINAL

In an industrial process ethanol C2H6o burns with Oz to produce heat.
C2H5OH + 3 o2 - 2 CO2 + 3 H20 + 8842 Joules
How many liters of CO2 are obtained from burning 0.28 moles of ethanol at STP (standard temperature and pressure? Express your result with 2 significant figures.

Answer 1

Volume of CO₂ obtained : 13 L

Further explanation

Reaction

C₂H₅OH + 3 O₂ ⇒ 2 CO₂ + 3 H₂0 + 8842 Joules

moles of ethanol=0.28

From equation, mol ratio ethanol : CO₂ = 1 : 2, so mol CO₂ :

`\tt (2)/(1)* 0.28=0.56`

Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure). At STP, Vm is 22.4 liters / mol.

Then volume of CO₂ :

`\tt V~CO_2=mol* 22.4=0.56* 22.4=12.544\approx 13~L`