Calculate values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) (a) Cr₂0₂2(aq) +1(aq) 1₂(s) + ³+ (aq) V P spontaneity: spontaneous not spontaneous balanced equation: chemPad (b) Cr₂0₂2(aq) + F(aq)-F₂(g) + ³+ (aq) spontaneity spontaneous not spontaneous balanced equation: chemPad 1x144 Help spontaneity: K) Hell) H (0) + H (9) Help balanced equation: chemPad spontaneous not spontaneous Help

Calculate the standard cell potential, ?∘cellEcell°, for the reaction shown. Use these standard reduction potentials.   Cu(s)+Ag+(aq)⟶Cu+(aq)+Ag(s)

Calculate the standard cell potential for the following galvanic cell. Ni(s)Ni(NO3)>(aq)||A9NO3(aq)|Ag(s)

3. Calculate the standard potentials for each of the cells at 298 K. Is each combination spontaneous as written? (a) Ag (s) | Ag + (aq) || Au *3 (aq) | Au (s) (b) Cu (s) | Cu +2 (aq) || Al *3 (aq) | Al (s)

Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and cathode.

a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc electrode immersed in ZnS saturated solution water. Sketch the galvanic cell, show the anode and cathode. Write the reactions occurring at the anode and cathode , as well as the general reaction of the galvanic element.Calculate the fem of this reaction.