This is an ignition.It forms CO2 and water.
CH4 + 2O2 gives CO2 and 2H2O.So 16g of CH4 react with 64g of O2.So 24g react with 96g of O2
Assuming complete combustion: CH4 + 2O2 --> 2H2O + CO2.
Take the balanced equation. CH4+2O2---->CO2+2H2O.So 2.8mol of CH4 need 5.6mol of O2.So O2 is limitting factor
CH4+O2 --- CO2+H2O... All that's missing - is the number 2 before the water molecule... CH4+O2 --- CO2+2H2O
Unbalanced CH4 + O2 = H2O + CO2 Balanced CH4 + 2O2 = 2H20 + CO2
The balanced equation is: CH4 + 2 O2 → CO2 + 2 H2O
When 85.0 g of CH4 are mixed with 160. g of O2 the limiting reactant is __________. CH4 + 2O2 → CO2 + 2H2O
CH4 + 2 O2 -> CO2 + 2 H2O So for every L of CH4 you need 2 L of O2 So for 50L of CH4 you need 100L O2
It is a combusion.Water and CO2 is produced
6 molecules of oxygen are needed to react with 3 methane molecules as one molecule of oxygen ( O2) are needed for methane gas.
Methane , CH4 , is a fuel that can react with O2 to yield CO2, H2O, and heat. CH4 (g) + O2 (g) ----> CO2 (g) + 2 H2O (g) + Heat
You should set up a balanced equation for the combustion of CH4 first: CH4 + 2 O2 --> CO2 + 2 H2O Now you see that for every 1 mole of CH4 you have 2 moles of O2. Therefore if you have 2.67 L of CH4, you'll have 5.34 L of O2. You can also assume it's at STP just to check, since it all cancels out in the end: 2.67L CH4 (1mol CH4/22.4L)(2mol O2/ 1 mol CH4)(22.4L/1mol O2)= 5.34L O2.