The standard cell potential (e°cell) for the reaction below is +1.10v. the cell potential for this reaction is v when the concentration of [cu2+]=1.0⋅10−5m and [zn2+]=2.5m. zn (s) + cu2+ (aq) → cu (s) + zn2+ (aq) the standard cell potential () for the reaction below is . the cell potential for this reaction is when the concentration of and (s) + (aq) (s) + (aq) 0.78 1.10 0.94 1.26 1.42

0.94 V

Explanation:

For the given chemical reaction :

Using Nernst equation :

where,

F = Faraday constant = 96500 C

R = gas constant = 8.314 J/mol.K

T = room temperature =

n = number of electrons in oxidation-reduction reaction = 2

= standard electrode potential of the cell = +1.10 V

= emf of the cell = ?

Now put all the given values in the above equation, we get:

The cell potential for this reaction is 0.94 V

i'm not sure

explanation:

i'll try whatever you got

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.