Okay so I need some help figuring out this problem balancing wise...
Heres the equation:
CH4(g) + O2(g) = CO2(g) + H2O (L)
Suppose 2 moles of methane (CH4) is allowed to react with 3 moles of oxygen...
So I can't figure out the product side!
2CH4(g) + 3O2(g) = ? CO2(g) + ? H2O(L)
Suppose 2 moles of methane... HELP!
Moderators: Xen, expert, ChenBeier
Hey
You see that if we are not specified with number of moles, we can see that the equation would be
CH4 + 2 O2 = CO2 + 2 H2O
Now you see every 1 mole of CH4 must react with 2 moles of O2 to give 1 mole of CO2 and two moles of H2O.
So CH4 Is half than oxygen. ANd CO2 is half than H2O
But we have 2 moles of CH4 so we wud need 4 moles of O2 but have only 3 moles
This means oxygen is limiting reagant. So overall prodcuts would be dependent on that. So, we would have
3/2 CH4 + 3O2 =3/2 CO2 + 3H2O
hope that helps,
You see that if we are not specified with number of moles, we can see that the equation would be
CH4 + 2 O2 = CO2 + 2 H2O
Now you see every 1 mole of CH4 must react with 2 moles of O2 to give 1 mole of CO2 and two moles of H2O.
So CH4 Is half than oxygen. ANd CO2 is half than H2O
But we have 2 moles of CH4 so we wud need 4 moles of O2 but have only 3 moles
This means oxygen is limiting reagant. So overall prodcuts would be dependent on that. So, we would have
3/2 CH4 + 3O2 =3/2 CO2 + 3H2O
hope that helps,
-Sharan