First balance Carbon (add 4 at right side, 4=4)
C4H10 --> 4 CO2 + H2O
Then balance Hydrogen (add 5 at right side, 10=5*2 )
C4H10 --> 4 CO2 + 5 H2O
Then balance Oxygen (add 6.5 O2 at left side, (4*2 + 5)right = 13 = (6.5*2)left
C4H10 + 6.5 O2 --> 4 CO2 + 5 H2O
Multply both siide by 2 to prevent halved quantities
2 C4H10 + 13 O2 --> 8 CO2 + 10 H2O
There is no way to balance that, because no matter how you group the molecules you're either creating oxygen atoms or destroying hydrogen atoms.We can fix that problem by assuming there's also oxygen present as a reactant and the water and carbon dioxide are products.
This is an extremely simple equation to balance, by the way, you should be able to do it trivially by accounting for the carbon and hydrogen and then working out how much oxygen you need.
Each butane (C4H10) has 4 carbon atoms, and will produce four CO2 molecules (using four O2 molecules to do so).
Each butane has 10 hydrogen atoms, and will produce five H2O molecules, using ... er ... okay, it's a LITTLE more complicated ... two and a half O2 molecules to do so. To fix this "half molecule" problem, we just multiply everything by two, and come up with
2 C4H10 + 13 O2 -> 10 H2O + 8 CO2
Checking, that's 2x4 = 8 carbon on the left and 8x1 = 8 carbon on the right, so that's good.
Hydrogen: 2 x 10 = 20 and 10 x 2 = 20 ... also good.
Oxygen: 13 x 2 = 26 and (10 x 1 = 10 plus 8 x 2 = 16) = 26.
Everything balances, so that must be the right equation.
the balanced equation is 2_C7H6O2+15_O2-->14_CO2+6_H2O
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
Every thing balanced first but O2. Leave that for last.
2C2H6 + 7O2 -> 4CO2 + 6H2O
Watch the carbohydrate and balance oxygen last.
(C4H10O)l + 6(O2)g = 4(CO2)g + 5(H2O)l
c3h6+o2---co2+h2o
2c2h6 + 7o2 -> 4co2 + 6h2o
2C2H6 + 7O2 -> 4CO2 + 6H2O
4C7H17 + 45O2 --> 28CO2 + 34H2O
This equation can not be balanced with the species present. Are you sure the species are correctly written?
C2H6O + O2 = C2H4O2 + H2O is balanced but not sure if this is what would happen
A hydrocarbon is C2H6.
C2H6 is ethane. It's one of the constituents of natural gas.
C2h6
2c4h10o + 13o2 -----> 8co2 + 10h2o
C2H5MgBr + H2 = C2H6 + MgBr2
2C2H6 + 7O2 --> 4CO2 + 6H2O
This equation can not be balanced with the species present. Are you sure the species are correctly written?
You mean balance it? 2C2H6 + 7O2 -> 4CO2 + 6H2O
C2H6O + O2 = C2H4O2 + H2O is balanced but not sure if this is what would happen
The reactants are C8H18 and oxygen.
A hydrocarbon is C2H6.
1molecule of C2H6 contains 2 carbon atoms
C2H6 is ethane. It's one of the constituents of natural gas.
Balanced equation first. 2C2H6 + 7O2 -> 4CO2 +6H2O I suspect C2H6 of limiting the reaction. 2 moles C2H6 (1.6 moles O2/2 moles C2H6) = 1.6 moles O2 left over and all of the C2H6 is consumed.
C2h6