Consider the following half-reactions Cu+eCu E-+0.521 V H₂O₂ +2e H₂O E = +1.776 V Question 2 Which of the following is the correct balanced chemical equation for a spontaneous redox reaction from the half-cell reactions above. OH,O, (aq) + 2 Cu()+2H,O (og)-2 Cu" (aq) + 2 H₂O(l) OH,O, (ag) +2 Cu(a) 2 Cu (aq) + 4H₂O(1) OH,O, (aq) +2 Cu() +21,0° (aq) - 2 Cu" (aq) + 4H₂O() O H₂O₂(aq) + Cu(a)+2H,O (ag) Cu (aq) + 4H₂O(l) Question 3 What is the potential (V) of the spontaneous, balanced redox reaction?

Consider these two entries from a fictional table of standard reduction potentials. X+ +3e X(s) E° = -1.94 V Y3+ +3e Y(s) E° = -0.31 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? V %3D 'cell

8)  Please answer in normal notation

I need help with all three questions PLEASE 1) What is the Eldeg cell for the following cell at 294 K? Zn(s) + X2 + (aq) → X(s) + Zn2+ (aq) K = 0.94 x10^4 2) When performing electrolysis of molten NaCl, how many grams of solid sodium are deposited at the cathode when a current of 32.6 A is applied for 1.23 hrs? 3) How many minutes would it take to deposit 4.95 g of Cu(s) from a solution of Cu(NO3)2 when using a current of 35.2 A ?