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 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.