Calculate the value of the cell potential, Ecell, for this reactión at 29 [1"] = 0.0050 M, and [Br2] = 1.0 M 12 (s) + 2 Br (aq) --> 21 (aq) + Br2 (aq) Note: The reaction shown above is the same as in the previous question; you'll need to use your answer to the previous question. EQUATIONS AND CONSTANTS E sell = E°cdll- (0.0592/n) log Q @ 25 °C R= 8.314 J/mol K AG a =-nFE°. F= 9.65 x 104 J/V•mol e cell AG rxn =-(RT)In K E"cell = (RT/nF) In K %3D For electrolysis: In (No/N) = kt 1A =1 C/s t12 0.693/k F = 9,65 x 104 C/mol e - 0.67 V + 0.99 V O + 0.23 V + 1.13 V - 0.45 V

Given the balanced electrochemical reaction below (M and N represent generic metals), what is the [M3*], in moles per liter, required to generate a cell potential (Ecell) of 0.584 V for this reaction at 58.1 °C when [N*] = 1.246 M? Enter your answer to the thousandths place. Do not include units. M(s) + 3N*(aq) –→ M3+(aq) + 3N(s) E°cell = 0.572 V

Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 4 significant digits. L (s) + 6H,0 (1) +5Zn²™ (aq) → 21IO, (aq)+ 12H" (aq)+ 5Zn (s) |kJ x10

The standard cell potential (E°cell) of the reaction below is -0.55 V. The value of A G° for the reaction is J/mol. 12 (s) + 2Br" (aq) → 21 (aq) + Br2 (1) 0.55 5.5 · 5. 10-6 1.1· 105 0.54 none of the above

Consider the following cell reaction: Ni(s) + 2 H*(? M). Ni?*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.118 volts, what is the pH of the hydrogen electrode? pH =

Consider the voltaic cell {Cu(s)|Cu2+(aq. 0.89 M)||Ag+(aq, 0.48 M)|Ag(s)}. What is E0cell and Ecell for this cell at 25 C?

The standard cell potential for the reaction shown here is .653 V. Calculate the cell potential at 25°C with [Hg^2+] = 0.0500 M, [V^2+] = 0.100 M, [Hg2^2+] = 0.00500 M and [V^3+] = %3D 0.0200 M. [Hg?+] do.o500 M [V2+] = 0.100 M H0.0500 M [Hg* = 0.00500 M [V³*] = 0.0200 M 2 Hg²+ (aq) + 2 V²+ (aq) = Hg2²+ (aq) + 2 V³+ (aq)