Question

Solid aluminum metal and diatomic bromine liquid react spontaneously to form a solid product. give the balanced chemical equation (including phases) that describes this reaction. indicate the phases using abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively.

Answer 1

Explanation:

Aluminium being metal reacts violently with liquid bromine. It is a highly exothermic reaction during which large amount of heat is released.

Aluminum when reacts with liquid bromine it gives aluminium bromide as a product.

The balanced chemical equation is given as:

$2Al(s) + 3Br_2(l)\rightarrow 2AlBr_3(s)$

According stoichiometry, 2 moles of aluminum metal react with 3 mole of liquid bromine to give 2 moles of aluminum bromide.

Answer 2

The balanced chemical equation for the reaction between aluminum and bromine is:

2Al (s) + 3Br₂ (l) —> 2AlBr₃ (s)

Chemical equation is simply a representation of chemical reaction with symbols and formula of the various reactants and products involved in the reaction.

However, chemical equation must be balanced in order to conform to the law of conservation of matter.

The equation for the reaction between aluminum and bromine is given below:

Al (s) + Br₂ (l) —> AlBr₃ (s)

The above equation can be balance as follow:

Al (s) + Br₂ (l) —> AlBr₃ (s)

There are 2 atoms of Br on the left side and 3 atoms on the right side. It can be balance by writing 3 before Br₂ and 2 before AlBr₃ as shown below:

Al (s) + 3Br₂ (l) —> 2AlBr₃ (s)

There are 2 atoms of Al on the right side and 1 atom on the left side. It can be balance by writing 2 before Al as shown below:

2Al (s) + 3Br₂ (l) —> 2AlBr₃ (s)

Therefore, the balanced chemical equation for the reaction between aluminum and bromine is:

2Al (s) + 3Br₂ (l) —> 2AlBr₃ (s)

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