Question

Balance this equation: \[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + }}{{\text{O}}_{\text{2}}} \to {\text{C}}{{\text{O}}_{\text{2}}}{\text{ + }}{{\text{H}}_{\text{2}}}{\text{O + energy}}\]

Answer 1

Hint: Balancing a chemical equation includes the making of the number of atoms of each compound same on both sides of the arrow. Many methods can be used to do this to make the mass of any element at the beginning of a reaction equal to its mass at the end of the reaction.

Complete step by step answer:
A balanced chemical equation is essential for the calculation and study of various factors involved in a reaction. It can be achieved through making the number of elements of compounds on both sides of the arrow equal. Here we have the equation as follows;
\[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + }}{{\text{O}}_{\text{2}}} \to {\text{C}}{{\text{O}}_{\text{2}}}{\text{ + }}{{\text{H}}_{\text{2}}}{\text{O + energy}}\]
Here we are using the trial and error method.
First, we are considering the number of carbon atoms in the reaction. Balancing its number, we can write the reaction as follows;
\[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + }}{{\text{O}}_{\text{2}}} \to 6{\text{C}}{{\text{O}}_{\text{2}}}{\text{ + }}{{\text{H}}_{\text{2}}}{\text{O + energy}}\]
Now the number of carbon atoms are same on both sides of the arrow. But the co-efficient 6 is applicable to all elements in \[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}\]. So now we are balancing the number of oxygen atoms and we get the equation as;
\[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + 6}}{{\text{O}}_{\text{2}}} \to 6{\text{C}}{{\text{O}}_{\text{2}}}{\text{ + }}{{\text{H}}_{\text{2}}}{\text{O + energy}}\]
The number of oxygen and hydrogen is not balanced on both sides and now we are adding a co-efficient to \[{{\text{H}}_{\text{2}}}{\text{O}}\] and then the equation becomes;
\[{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + 6}}{{\text{O}}_{\text{2}}} \to 6{\text{C}}{{\text{O}}_{\text{2}}}{\text{ + 6}}{{\text{H}}_{\text{2}}}{\text{O + energy}}\]
Now we will analyse the number of each element on both sides of the reaction;

${\text{Element}}\;{\text{ Reactant Side Product Side}} \\
{\text{ C 6 6}} \\
{\text{ H 12 12}} \\
{\text{ O 18 18}} \\
$
Hence the number of elements on both sides are now equal.


Additional Information:
The Law of Conservation of Mass dates was discovered in 1789 after Antoine Lavoisier discovered that mass can neither be created nor be destroyed in a chemical reaction and that the total mass of reactants and products will be the same at any point of time.

Note: Balancing a chemical equation includes the use of law of conservation of mass which states that the mass of reactants reacted will be equal to the mass of products formed. It was discovered after Lavoisier’s theory of conservation of mass in chemical reactions.