How many grams of 〖Cl〗_2 is produced from 15.8 g of 〖KMnO〗_4 and 50mL of 10 M HCl according to the reaction
2KMnO_4+16HCl→2KCl+2MnCl_2+8H_2 O+5Cl_2?
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Explanation:
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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.
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