I only need the answer to part D)...hint: the answer is not 1.93 x 10^5 c The ov

ID: 918456 • Letter: I

Question

I only need the answer to part D)...hint: the answer is not 1.93 x 10^5 c

The overall cell reaction occurring in an alkaline battery is:

Zn(s) + MnO2(s) + H2O(l) ---> ZnO(s) + Mn(OH)2(s)

a) How many moles of electrons flow per mole of reaction?............answer: 2. Mol e-Note:

b) If 6.09g of zinc is oxidized, how many grams of manganese dioxide and of water are consumed?

Grams MNnO2 ???? answer : 8.092 g

grams H2O ????? answer: 1.676 g

c) What is the total mass of reactants consumed in part (b)?.......grams??? answer: 15.858 g

d) How many coulombs are produced in part (b)?.....I need this answer in scientific notation.

repeat the answer is NOT 1.93 x 10^5 (both of these parts are wrong....the 1.93 and the 10^5)

thank you

Atomic weight of Zinc= 66

Molecular weight of MnO2= 87

Molecular weight of water =18

Moles of Zinc =6.09/66= 0.092273 moles

Moles of MnO2 consumed =0.092273 moles = 0.092273*87= 8.023 gm and moles of water = 0.092273 moles =0.092273*16= 1.67 gms

The ionic forms of reaction is Zn + Mn+4--à Zn+2 + Mn+2

Hence there are two moles of electrons exchanged for every mole of reactants

Charge of one electron =1.6*10-19

Columba produced= 1.6*10-19 *2 =3.2*10-19 coulombs