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Olin [163]
2 years ago
9

How do you make these equations balanced?

Chemistry
1 answer:
Sedaia [141]2 years ago
3 0

Explanation:

both iron and sulphur in FeS2 undergo a change in oxidation state.

O2° -->2O degree2- Total decrease = 2×2=4

So, 4FeS2+11O2 --> 2Fe2O3+8 SO2

Hence, balanced

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Give the o.N. Of each of the elements magnesium and oxygen in the reactants and in the products 2Mg + O2=2MgO
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Answer:

2Mg^0 + O_2^0\rightarrow2Mg^{2+}O^{2-}

Explanation:

Hello there!

In this case, according to the rules for the oxidation states in chemical reactions, it is possible to realize that lone elements have 0 and since magnesium is in group 2A, it forms the cation Mg⁺² as it loses electrons and oxygen is in group 6A so it forms the anion O⁻²; therefore resulting oxidation numbers are:

2Mg^0 + O_2^0\rightarrow2Mg^{2+}O^{2-}

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