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3 years ago

Consider the redox reaction below.

Chemistry

1 answer:

elixir [45]3 years ago

4 0

Explanation:

Fe²⁺ + 2e⁻ → Fe

In a reduction half, the oxidizing agent is getting reduced. Such ion is donating electrons.

In a reduction process:

there is removal of oxygen from a specie
addition of hydrogen to a specie
gain of electron by an atom
decrease in oxidation number of an atom
decrease in number of electronegative atoms surrounding the element in changing from reactants to products.

Learn more:

Redox reactions brainly.com/question/2890416

#learnwithBrainly

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3 years ago

Which reactant is limiting? Show work

fenix001 [56]

Answer:

1. Iodine is the limiting reactant

2. $6molAlI_3$

Explanation:

1. Balanced chemcial equation:

$2Al+3I_2\rightarrow 2AlI_3$

2. Theoretical mole ratio

It is the ratio of the coefficients of the reactants in the balanced chemical equation:

$\dfrac{2molAl}{3molI_2}$

3. Actual ratio

It is ratio of the moles available to reat:

$\dfrac{9molAl}{9molI_2}$

4. Comparison

$\dfrac{9molAl}{9molI_2}>\dfrac{2molAl}{3molI_2}$

Then, there are more aluminum available than what is needed to react with the 9 moles of iodine, meaning that the aluminum is in excess and the iodine will react completely, being the latter the limiting reactant.

Conclusion: iodine is the limiting reactant.

5. How much aluminum iodide will be produced?

Use the theoretical mole ratio of aluminum iodide to iodide:

$\dfrac{2molAlI_3}{3molI_2}\times 9molI_2=6molAlI_3\leftarrow answer$

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