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AlladinOne [14]
3 years ago
5

What is the oxidation state of each element in the species Mn(ClO4)3?

Chemistry
2 answers:
gayaneshka [121]3 years ago
7 0
The oxidation state of the compound Mn (ClO4)3 is to be determined in this problem. For oxygen, the charge is 2-, the total considering its number of atoms is -24. Mn has a charge of +3. TO compute for Mn, we must achieve zero charge overall hence 3+3x-24=0 where x is the Cl charge. Cl charge, x is +7. 
Ronch [10]3 years ago
4 0

Answer:

Mn: 3+

Cl: 7+

O: 2-

Explanation:

1) Compound given: Mn [ClO₄]₃

2) Initially you only know the oxidation state of O, since it is always 2-, except when it form peroxides, which is not the case.

3) So, you do not know the oxidation states neither of the Mn nor of the Cl, and you need some more information.

You might start from the ion [ClO₄] but you do not know its charge.

This ion comes from one of the oxoacids formed by Cl. Those are four different acids. These are them:

i) Oxidation state 1+: Cl₂O + H₂O → H₂Cl₂O₂ = HClO ⇒ ion ClO⁻

ii) Oxidation state 3+: Cl₂O₃ + H₂O → H₂Cl₂O₄ = HClO₂ ⇒ ion ClO₂⁻

iii) Oxidation state 5+: Cl₂O5 + H₂O → H₂Cl₂O₆ = HClO₃ ⇒ ion ClO₃⁻

iv) Oxidation state 7+: Cl₂O₇ + H₂O → H₂Cl₂O₈ = HClO₄ ⇒ ion ClO₄⁻

Finally, we have that our ion is ClO₄⁻ and the oxidation state of Cl is 7+.

4) Now you just have to find the oxidation state of Mn, for which you make a balance of charges:

Mn [ClO₄]₃

Since, the ion ClO₄⁻ has 1 negative charge, and there are 3 ions the total negative charge is 3-. Since the compound is neutral, you conclude that Mn has oxidation state 3+.

That according to this balance: 1(3+) + 3(1-) + 3 - 3 = 0.

5) Summarizing, the oxidation states are:

Mn: 3+

Cl: 7+

O: 2-



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Answer:

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Explanation:

Step 1:

The balanced equation for the reaction of CaCl2 to produce CaCO3. This is illustrated below:

When CaCl2 react with Na2CO3, CaCO3 is produced according to the balanced equation:

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Step 2:

Conversion of 85g of CaCO3 to mole. This is illustrated below:

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Determination of the number of mole of CaCl2 needed to produce 85g (i.e 0. 85 mole) of CaCO3.

This is illustrated below :

From the balanced equation above,

1 mole of CaCl2 reacted to produced 1 mole of CaCO3.

Therefore, 0.85 mole of CaCl2 will also react to produce 0.85 mole of CaCO3.

From the calculations made above, 0.85 mole of CaCl2 is needed to produce 85g of CaCO3

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