The coefficients in the order CH₄, O₂, CO₂, and H₂O, are 1,2,1,2
The equation becomes:
CH₄ (g) + 2O₂ (g) -> CO₂ (g) + 2H₂0 (g)
Complete combustion of hydrocarbon with oxygen will be obtained by CO₂ and H₂O compounds.
If O is insufficient there will be incomplete combustion produced by CO and H and O
Hydrocarbon combustion reactions (specifically alkanes)
[tex]\large {\boxed {\bold {C_nH _ (_2_n _ + _ 2_) + \frac {3n + 1} {2} O_2 ----> nCO_2 + (n + 1) H_2O}}}[/tex]
Equalization of chemical reaction equations can be done using variables.
Steps in equalizing the reaction equation:
For gas combustion reaction which is a reaction of hydrocarbons with oxygen produces CO₂ and H₂O (water vapor). can use steps:
Balancing C atoms, H and last atoms O atoms
Methana combustion reaction
CH₄ (g) + O₂ (g) -> CO₂ (g) + H₂0 (g)
We give the most complex compounds, namely Methane, we give the number 1
So the reaction becomes
CH₄ (g) + aO₂ (g) -> bCO₂ (g) + cH₂0 (g)
C atom on the left 1, right b, so b = 1
H atom on the left 4, right 2c, so 2c = 4 ---> c = 2
Atom O on the left 2a, right 2b + c, so 2a = 2b + c
2a = 2.1 + 2
2a = 4
a = 2
The equation becomes:
CH₄ (g) + 2O₂ (g) -> CO₂ (g) + 2H₂0 (g)
the combustion of octane in gasoline
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Keywords: methane, combustion, hydrocarbons, equalization of reaction equations
The balanced chemical equation is as follows:
[tex]{\text{C}}{{\text{H}}_4}\left( g \right) + 2{{\text{O}}_2}\left( g \right) \to {\text{C}}{{\text{O}}_{\text{2}}}\left( g \right) + 2{{\text{H}}_{\text{2}}}{\text{O}}\left( g \right)[/tex]
The coefficients of [tex]{\mathbf{C}}{{\mathbf{H}}_{\mathbf{4}}}[/tex] is [tex]\boxed1[/tex], [tex]{{\mathbf{O}}_{\mathbf{2}}}[/tex] is [tex]\boxed2[/tex], [tex]{\mathbf{C}}{{\mathbf{O}}_{\mathbf{2}}}[/tex] is [tex]\boxed1[/tex] and [tex]{{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}[/tex] is [tex]\boxed2[/tex]
Further Explanation:
The chemical reaction that contains equal number of atoms of the different elements in the reactant as well as in the product side is known as balanced chemical reaction. The chemical equation is required to be balanced to follow the Law of the conservation of mass.
Combustion reaction is the reaction in which the reactant reacts with molecular oxygen to form carbon dioxide and water molecule. Molecular oxygen acts as the oxidizing agent in these reactions. The large amount of heat is released and therefore combustion reactions are exothermic reaction.
The steps to balance a chemical reaction are as follows:
Step 1: Complete the reaction and write the unbalanced symbol equation.
In the combustion reaction, [tex]{\text{C}}{{\text{H}}_4}[/tex] reacts with [tex]{{\text{O}}_2}[/tex] to form [tex]{\text{C}}{{\text{O}}_{\text{2}}}[/tex] and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex]. The physical state of [tex]{\text{C}}{{\text{H}}_4}[/tex] is gas, [tex]{{\text{O}}_2}[/tex] is gas, [tex]{\text{C}}{{\text{O}}_{\text{2}}}[/tex] is gas and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] is gas. The unbalanced chemical equation is as follows:
[tex]{\text{C}}{{\text{H}}_4}\left(g\right)+{{\text{O}}_2}\left(g\right)\to{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)[/tex]
Step 2: Then we write the number of atoms of all the different elements that are present in a chemical reaction in the reactant side and product side separately. There is one carbon atom on both the reactant and product side. 2 oxygen atoms are present on the reactant side while 3 oxygen atoms are present on the product side. The number of hydrogen atoms on the reactant and product sides is 4 and 2 respectively. (Refer table in the attached image).
Step 3: Initially, we try to balance the number of other atoms of elements except for carbon, oxygen, and hydrogen by multiplying with some number on any side but in the combustion reaction there is only carbon, hydrogen and oxygen atom.
Step 4: After this, we balance the number of atoms of oxygen and then carbon atom followed by hydrogen atoms. To balance the number of atoms of oxygen and hydrogen, we have to multiply [tex]{{\text{O}}_2}[/tex] by 2 and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] by 2. The chemical equation is as follows:
[tex]{\text{C}}{{\text{H}}_4}\left(g\right)+2{{\text{O}}_2}\left(g\right)\to{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)[/tex]
Step 5: Finally, we check the number of atoms of each element on both sides. If the number is same then the chemical equation is balanced. The balanced chemical equation is as follows:
[tex]{\text{C}}{{\text{H}}_4}\left(g\right)+2{{\text{O}}_2}\left( g \right) \to{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)[/tex]
The coefficients of [tex]{\text{C}}{{\text{H}}_4}[/tex] is 1, [tex]{{\text{O}}_2}[/tex] is 2, [tex]{\text{C}}{{\text{O}}_{\text{2}}}[/tex] is 1 and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] is 2.
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Answer details:
Grade: High School
Subject: Chemistry
Chapter: Chemical reaction and equation
Keywords: Balancing, CH4, O2, CO2, H2O, phases, physical state, solid, liquid, gas, aqueous, coefficients, and combustion reactions.
