# In the equation 16HCl + 2KMnO4 ->2KCl + 2MnCl2 + 5Cl2 +8H2O if 1 mole of KMnO4 how many moles of H2O produced? How many grams of KCl produced with 1.0 mol KMnO4 16HCl + 2KMnO4  ------> 2KCl + 2MnCl2 + 5Cl2 + 8H2O

The equation is balanced and gives proper stoichiometry. This is a redox reaction involving HCl and KMnO4.

According to stoichiometry of the reaction 2 moles of KMnO4 will produce 8 moles of H2O. That means 1 mol of KMnO4...

16HCl + 2KMnO4  ------> 2KCl + 2MnCl2 + 5Cl2 + 8H2O

The equation is balanced and gives proper stoichiometry. This is a redox reaction involving HCl and KMnO4.

According to stoichiometry of the reaction 2 moles of KMnO4 will produce 8 moles of H2O. That means 1 mol of KMnO4 will produce exactly 4 moles of H2O  (since 8/2 = 4).

In the same manner, 2 moles of KMnO4 will produce 2 moles of KCl according to stoichiometry. Therefore 1 mol of KMnO4 will produce 1 mol of KCl. To find the mass of KCl produced we need to find the molar mass of KCl.

Molar mass of KCl = Molar mass of K + Molar mass of Cl

= 39 + 35.5

= 74.5 g per mol

The mass of KCl produced = 1 mol x 74.5 g per mol

= 74.5 g.

Therefore 1 mol of KMnO4 will produce 74.5 g of KCl.