Question

demonstration 3: how do you balance an equation?
what will the coefficients be for each molecule when this equation is balanced?
prediction and reasoning
h₂o → h₂ + o₂
actual
h₂o → h₂ + o₂
reactant side product side
2 h 2
1 o 2
conclusion
explain how balanced equations show conservation of mass.
application
the following equation is balanced, but not simplified. what are the coefficients when the equation is balanced using the smallest, whole - number coefficients? support your answer.
4 co → 2 c + 2 co₂

Explanation:

Step1: Balance the water - decomposition equation

The un - balanced equation is $H_2O
ightarrow H_2 + O_2$. On the reactant side, we have 1 oxygen atom and 2 hydrogen atoms, and on the product side, 2 oxygen atoms and 2 hydrogen atoms. To balance the oxygen atoms, we put a 2 in front of $H_2O$ and a 2 in front of $H_2$. The balanced equation is $2H_2O
ightarrow 2H_2+O_2$. The coefficients are 2 for $H_2O$, 2 for $H_2$ and 1 for $O_2$.

Step2: Simplify the carbon - monoxide decomposition equation

The given equation is $4CO
ightarrow 2C + 2CO_2$. We can divide each coefficient by 2. The simplified balanced equation is $2CO
ightarrow C + CO_2$. The coefficients are 2 for $CO$, 1 for $C$ and 1 for $CO_2$.

Answer:

For $H_2O
ightarrow H_2 + O_2$, the coefficients are 2, 2, 1. For $4CO
ightarrow 2C + 2CO_2$, the simplified coefficients are 2, 1, 1.