Methane, the principal component of natural gas, is used for heating and cooking.?

Question

The combustion process is:
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)
If 15.0 moles of CH4 are reacted, what is the volume of CO2 (in liters) produced at 23.0 degrees C and 0.985 atm?


.. the answer is 370 L .. just dont know how to get it! please help!

Answer 1

this is easy:
1 mol ch4 creates 1 mol co2, so 15 mol ch4 creates 15 mol co2.

in STP, 1 mol co2 is 22.4 L. so 15 mol is 15*22.4=336 L

then u apply the P1*V1/T1=P2*V2/T2 equation.

P1=1 atm
V1=336 L
T1=273 K

P2=.985 atm
T2=273+23=296 K
V2=?

After putting the values in the equation, u get V2=369.855 L, which is nearly 370 L

Answer 2

15 moles of CH4 will burn to form 15 moles of CO2.  What they're asking is for you to find the volume of 15 moles of CO2 at that temperature/pressure according to Boyle's Law.

PV = nRT

You have to convert temperature to absolute (Kelvin) but if you have R in the correct units (atmosphere-liters per mol Kelvin) the answer falls out directly.  Otherwise you have to convert units (atmospheres to Pascals or the like).

Answer 3

Use the Ideal Gas Law PV=nRT
n=15mol;P=.985atm;R=.08314,T=296.15K

V = 374.953L

Answer 4

ANY TYPE OF NATURAL GAS IS PRESSURIZED BY VOLUME SO FIG-UAR VOLUME BY DEGREESE