classify each reaction and balance the equation Al(OH)3--> Al2O3 + H2O
Do you understand the principle behind naming reactions this way?
When A + B ==> C it is a synthesis reaction. Synthesis means making something and you are adding two things to make one thing.
C==> A + B is the reverse of synthesis. It is a decomposition reaction. One thing becomes more than one.
A + BC ==> B + AC is a single replacement. A replaced B.
AB + CD ==> AC + BD is a double replacement. The two compounds (AB and CD just changed places; that is, A replaced C and D replaced B.
Now you know which yours is.
To classify the reaction, we can look at the chemical formula and determine the type of reaction taking place. In this case, we have:
Al(OH)3 → Al2O3 + H2O
This is an example of a decomposition reaction because a single reactant (Al(OH)3) breaks down into two or more products (Al2O3 and H2O).
To balance the equation, we need to ensure that there are an equal number of atoms on both sides of the equation. To do this, we can follow these steps:
1. Count the number of atoms on each side of the equation:
Al: 1 Al atom on the reactant side, 2 Al atoms on the product side.
O: 3 O atoms on the reactant side, 3 O atoms on the product side.
H: 3 H atoms on the reactant side, 2 H atoms on the product side.
2. Start by balancing the atoms that appear in the fewest compounds. In this case, it's the H atoms, so let's balance those first:
Add a coefficient of 3 in front of H2O on the product side to have 6 H atoms on both sides:
Al(OH)3 → Al2O3 + 3H2O
3. Now, let's balance the Al and O atoms:
Al: 1 Al atom on the reactant side, 2 Al atoms on the product side.
Add a coefficient of 2 in front of Al(OH)3 on the reactant side to match the number of Al atoms on both sides:
2Al(OH)3 → Al2O3 + 3H2O
O: 3 O atoms on the reactant side, 3 O atoms on the product side.
Add a coefficient of 3 in front of Al2O3 on the product side to match the number of O atoms on both sides:
2Al(OH)3 → Al2O3 + 3H2O
Now the equation is balanced:
2Al(OH)3 → Al2O3 + 3H2O