Electrochemistry

hello

the first question

Cu²⁺+2e--->Cu

E_cell=E⁰_cell - .0592log1[Cu²⁺]
now replace [Cu²⁺] by [Cu²⁺]10

E'_cell=E⁰_cell - .0592log10[Cu²⁺]

subtract both

hence decrease by .0592=29.5 mV answer is C

@cool rocks
u mean (d)?

2nd question

at equilibrium ΔG=0 so is E_cell

now write nernst equation and solve the question

3.
we have ΔG=-2.303RTlogK
also ΔG=-nFE
equating the above, 2.303 x 8.314(J/molK) x 298(k) x log(2.69x10¹²) = 2 x 96500(F\mol) x E
so you can calculate E

so are you getting exact .1836V as answer??

the above working should give the correct ans. i havent calculated