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Romashka [77]
2 years ago
9

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of h2c2o4 and h2o in th

e balanced reaction? mno4⁻(aq) h2c2o4(aq) → mn2 (aq) co2(g)
Chemistry
1 answer:
postnew [5]2 years ago
8 0

The balanced redox reaction, if it occurs in acidic solution, is

5C₂O₄²⁻(aq) + 2MnO₄⁻(aq) + 16H⁺-----> 10CO₂(g) + 2Mn²⁺(aq) + 8H₂O(l)

<h3>What are redox reaction?</h3>

Redox reactions are those in which loss and again of electrons occur.

To balance the redox reaction, we must first break the whole reaction into half equations;

Oxidation half equation

\rm 5C_2O4^2^-(aq) + 10e + 8H^+----- > 10CO_2(g) + 4H_2O(l)

Reduction half equation

\rm 2MnO_4^- (aq) + 10e + 8H^+----- > 2Mn^2+(aq) + 4H_2O(l)

Now combine both the reactions

\rm 5C_2O_4^2-(aq) + 2MnO4^- (aq) + 16H^+----- > 10CO_2(g) + 2Mn^2+(aq) + 8H_2O(l)

Thus, the coefficient of H₂C₂O₄ is 5 and that of water is 8.

Learn more about redox reactions

brainly.com/question/13293425

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These types of molecules are called hydrates. They have a certain number of moles attached to the salt. Their characteristic is being hygroscopic. That means that when they are exposed to air, they readily solvate. 

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Explanation:

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A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are
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<h3>Answer:</h3>

82.11%

<h3>Explanation:</h3>

We are given;

  • Theoretical mass of the product is 137.5 g
  • Actual mass of the product is 112.9 g

We are supposed to calculate the percentage yield

  • We need to know how percentage yield is calculated;
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