I obtained this reaction from Wikipedia. Compare with the reaction in your text/notes. If not the same you will need to adjust my post.
Zn(s) + 2MnO2(s) is in equilibrium with ZnO(s) + Mn2O3(s) [e° = 1.43 V]
molsZn = grams Zn/atomic mass Zn
Using the coefficients in the balanced equation, convert mols Zn to mols MnO2.
Now convert mols MnO2 to g. g = mols x molar mass.
#2. mols Zn x 6.02E23 atoms/mol x 2e/atom x 1.6E-19 C/electron = ?
During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.
a) What mass of MnO2 is reduced at the cathode during this discharge?
b) How many Coulombs of electrical charge are transferred from Zn to MnO2?
1 answer