The balanced equation for complete combustion of heptane is
C7H16 + 11O2 ---(ignition)---> 7CO2 + 8H2O.
For each moelcule of heptane, you would need 11 molecules of oxygen gas.
Heptane has the molecule formula: C7H16
When burning things such as alkanes the products are most likely H2O and CO2.
So lets make a reaction equation for this.
C7H16 + O2 --> CO2 + H2O
As you can see the amount of atoms before and after the reaction arrow dont match, just play with the numbers till the number of carbon, hydrogen and oxygen atoms before and after the arrow are the same.
C7H16 + 9 O2 --> 7 CO2 + 8 H2O
This is the reaction, and as you can see, 1 mole of heptane reacts with 9 moles of O2 to form 7 moles of CO2 and 8 moles of H2O.
To determine how many moles of Oxygen is needed for the combustion of 1 mole of Butane, we start with a balanced chemical equation. Butane is C4H10:
2 C4H10 + 13 O2 ---> 8 CO2 + 10 H2O
From the equation, we find that 2 moles of butane require 13 moles of oxygen to combust; therefore, one mole of butane requires 6.5 moles of oxygen.
If the combustion is complete, the equation for the reaction is:
2 C3H10 + 11 O2 -> 6 CO2 + 10 H2O.
Therefore, the moles of oxygen needed will always be 11/2 times the number of moles of propane reacted.
11 moles of oxygen are needed for the complete combustion of heptane.
C7H16 + 11O2 --> 7CO2 + 8H2O
The chemical reaction of this combustion is:
2 C6H14 + 19 O2 = 12 CO2 + 14 H2O
Answer: 9,5 moles of oxygen are neede.
The chemical reaction is;
2 C6H14 + 19 O2 = 12 CO2 + 14 H2O
For one mole o f hexane 9,5 moles of oxygen are necessary.
11
When the combustion is complete, the balanced equation is: C7H16 + 11 O2 -> 7 CO2 + 8 H2O.
Oxygen is a required reactant in a combustion reaction - without oxygen, you do not have combustion. If you combine a hydrocarbon with oxygen and add heat, you will cause a combustion reaction that results in carbon dioxide and water being formed (provided there was complete combustion).
C7H16+11O2 = 7CO2+8H2O is the balanced equation for the complete combustion of heptane.
No moles of oxygen are produced by complete combustion of propane. Oxygen is CONSUMED, not produced. For combustion of 4 moles of propane, it will use 20 moles of oxygen.
burning in oxygen ensures complete combustion
When the combustion is complete, the balanced equation is: C7H16 + 11 O2 -> 7 CO2 + 8 H2O.
Oxygen is a required reactant in a combustion reaction - without oxygen, you do not have combustion. If you combine a hydrocarbon with oxygen and add heat, you will cause a combustion reaction that results in carbon dioxide and water being formed (provided there was complete combustion).
C7H16+11O2 = 7CO2+8H2O is the balanced equation for the complete combustion of heptane.
No, oxygen is required for combustion to take place.
More oxygen is used in a complete combustion.
For the complete combustion reaction, the equation is: C7H16 (l) + 11 O2 (g) => 7 CO2 (g) + 8 H2O (g).
No. Oxygen is required for combustion. Mercury is not involved.
in complete combustion the amount of oxygen is higher/more than the amount of oxygen in incomplete combustion. Heat needs oxygen.
oxygen
Complete combustion of a hydrocarbon yields carbon dioxide & water; incomplete combustion yields carbon monoxide & water. By having excess oxygen you have enough oxygen to ensure complete combustion. For example the combustion of methane (CH4):complete combustion: CH4 + 2O2 --> CO2 + 2H2Oincomplete combustion: CH4 + 1.5O2 --> CO + 2H2OAs you can see you need a 1/2 mole less of oxygen for the incomplete combustion of methane. So as long as you have twice the amount (in terms of moles) of oxygen as methane you will ensure complete combustion. So anything in excess of that will also ensure complete combustion.
No moles of oxygen are produced by complete combustion of propane. Oxygen is CONSUMED, not produced. For combustion of 4 moles of propane, it will use 20 moles of oxygen.
what is the mass in grams of oxygen, is needed to complete combustion of 6 L of methane?