balance the reaction, do not leave any fractions, dont leave anything blank, then answer the questions about the reaction
__1__ al₂o₃ → __2__ al + __3__ o₂
this is an __4__ reaction.
is this a redox reaction? (yes/no)__5__, because al⁺³ is reduced to al⁰, and because o⁻² is __6__ to o⁰.
will the reaction happen as it is written? (yes/no)__7__, because o₂ is reactive and will not form. the reverse reaction would happen.
a. 1 b. 2 c. 3 d. 4 e. 5 f. 6 g. 7 h. 8 i. 9
j. 10 k. 12 l. 14 m. 16 n. 18 o. 20 p. 22 q. 24 r. 26
s. 28 t. synthesis u. decomposition v. single displacement w. double displacement x. neutralization y. yes z. no aa. reactive bb. stable cc. oxidized dd. reduced

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Accepted Answer

# Explanation:
## Step1: Balance the chemical equation
For the reaction $Al_2O_3
ightarrow Al + O_2$, we need to balance the number of atoms.
- For aluminum ($Al$): There are $2$ $Al$ atoms in $Al_2O_3$. Let the coefficient of $Al_2O_3$ be $a$, of $Al$ be $b$, and of $O_2$ be $c$. The number of $Al$ atoms: $2a = b$.
- For oxygen ($O$): There are $3$ $O$ atoms in $Al_2O_3$, so $3a=2c$.
If we take $a = 2$, then $b = 4$ (since $2a=b$) and $c = 3$ (since $3a = 2c$, $3\times2=2c$, $c = 3$). The balanced equation is $2Al_2O_3
ightarrow4Al + 3O_2$.

## Step2: Identify the type of reaction
In a decomposition reaction, a single compound breaks down into two or more simpler substances. Here, $Al_2O_3$ breaks down into $Al$ and $O_2$, so it is a decomposition reaction.

## Step3: Determine if it is a redox reaction
In a redox reaction, there is a change in oxidation states.
- For $Al$: In $Al_2O_3$, the oxidation state of $Al$ is $+ 3$ (since $O$ has an oxidation state of $-2$ and for $Al_2O_3$, $2x+3\times(- 2)=0$, $x = +3$), and in $Al$ (elemental form) it is $0$. So $Al$ is reduced ($Al^{+3}
ightarrow Al^{0}$).
- For $O$: In $Al_2O_3$, the oxidation state of $O$ is $-2$, and in $O_2$ (elemental form) it is $0$. So $O$ is oxidized ($O^{-2}
ightarrow O^{0}$). Since there is both oxidation and reduction, it is a redox reaction.

## Step4: Determine if the reaction will happen as written
$O_2$ is a very reactive gas. The forward reaction $2Al_2O_3
ightarrow4Al + 3O_2$ requires a lot of energy (high - temperature electrolysis for example in industrial processes like Hall - Heroult process). In a simple sense (without considering extreme conditions like high - temperature electrolysis),  $O_2$ is reactive and the reverse reaction $4Al + 3O_2
ightarrow2Al_2O_3$ (a synthesis reaction) is more spontaneous. So the reaction as written (forward direction without proper conditions) will not happen easily.

# Answer:
1. B. 2
2. D. 4
3. C. 3
4. U. decomposition
5. Y. yes
6. CC. oxidized
7. Z. no

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Question

Explanation:

Step1: Balance the chemical equation

Step2: Identify the type of reaction

Step3: Determine if it is a redox reaction

Step4: Determine if the reaction will happen as written

Answer: