a)
Mn(s) + Cu2+(aq) ------> Mn2+(aq) + Cu(s)
b)
current = charge / time
charge = current * time
= 1.34 * 1.99 *60*60
charge = 9599.76 C
1 mole of electron contain 96485 C charge
no of moles of electron = 9599.76 / 96485 = 0.0995 mol
c)
moles of Mn oxidized = 0.0995 / 2 = 0.0497 mol
mass of Mn oxidized = 0.0497 * 54.938 = 2.73 g
so
change in mass of Mn electrode = 2.73 g is decrease
d)
moles of Cu Reduced = 0.0995 / 2 = 0.0497 mol
mass of Cu Reduced = 0.0497 * 63.546 = 3.158 g
change in mass of Copper electrode = 3.158 g is increase
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