HI + 2 KMnO4 + 3 H2SO4 - -> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O55. According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4? A) 20B) 10C) 8.0D) 5.0E) 2.5

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London Price

Chemistry

5 July, 02:39

HI + 2 KMnO4 + 3 H2SO4 - -> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O55. According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4? A) 20B) 10C) 8.0D) 5.0E) 2.5

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Cedric Duffy · Answer 1

B) 5

Explanation:

The complete balanced equation is discribed bellow:

10HI + 2 KMnO4 + 3H2SO4 → 5I2 + 2 MnSO4 + K2SO4 + 8 H2O

The amount of atoms of an element should be the same in the reactants and in the products. Therefore, if we have 2.5I2 in the product, it means that we need 5 atoms of I in the reactant. Since the only source of I in the reactant is HI, we need 5.0 mol of HI to produce 2.5 mol of I2.

The final balanced equation would be:

5 HI + 1 KMnO4 + 1.5 H2SO4 → 2.5 I2 + 1 MnSO4 + 0.5 K2SO4 + 4 H2O

The remaining KMnO4 and H2SO4 would not be consumed.