Question

Methane burns in air to produce carbon dioxide and water: CH4(g) + 2 O2(g) --> CO2 (g) +2 H2O (l) What volume of carbon dioxide, at 1 atm pressure and 112°C, will be produced when 80.0 grams of methane is burned?

Answer 1

`V=157.91L`

Step-by-step explanation:

Hello,

Based on the stoichiometry, the produced moles of carbon dioxide are computed via:

`n_(CO_2)=80.0gCH_4*(1mol CH_4)/(16gCH_4) *(1molCO_2)/(1molCH_4)=5mol CO_2`

Now, by using the ideal gas law and subsequently solving for the volume we get:

`V=(nRT)/(P)= (5mol*0.082(atm*L)/(mol*K)*385.15K)/(1atm)=157.91L`

Best regards.