In a voltaic cell based on the Cu-Zn reaction

Zn(s) + Cu2+ (aq) --> Cu(s) + Zn2+ (aq)
there is exactly 1 mole of each reactant and product. A second cell based on the Cd-Cu cell reaction
Cd(s) + Cu2+ (aq) --> Cu(s) + Cd2+ (aq)
also has exaclty 1 mole of each reactnat and product. Which of the following statements about the two cells is true?

A) The quantities of electrical energy that they can produce are the same
B) The masses of their elctrodes are the same
C) The quantities of electrical charge that are they can produce are the same
D) Their cell potentials are the same

The quantities of electrical charge that are they can produce are the same

Explanation:

The quantity of electrical charge produced by an electrochemical cell is given by

Number of moles of electrons × Faraday's constant.

since the number of moles of electrons involved in the two electrochemical reactions are the same (2 moles of electrons each) then the charge that they can produce will also be the same.

Hence the answer.

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2