I only need the answer to part D)...hint: the answer is not 1.93 x 10^5 c nor 3.

ID: 918587 • Letter: I

Question

I only need the answer to part D)...hint: the answer is not 1.93 x 10^5 c nor 3.2 x 10^-19

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)

nor is the the answer 3.2 x 10^-19 ,,,both parts were wrong here as well

Thank you...

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

2 mol e- are exchanged for every 1 mol reaction.

No of moles reacted = g of Zn reacted/molar mass of Zn = 6.09/65.38 = 0.093 mole

Total no of moles of electrons flowed = 0.093 * 2 = 0.186 Mole

1 mole of electrons carry charge = 96485 C

Charge carried by 0.186 mole of electron = 0.186 * 96485 = 17946 C