The standard reduction potentials for two pairs of redox species are shown below. What is the reading on a potentiometer (in volts) under standard conditions if these two reactions are used to design the following cell:  Sn (s) | Sn2+ (aq) || Fe2+ (aq) | Fe (s) Half-Reactions Sn2+ (aq) + 2e- → Sn(s)         E° = -0.14 V Fe2+ (aq) + 2e- → Fe (s)        E° = -0.44 V

Sn(s) | Sn2+ (aq, 1.8 M) || Agt(aq, 0.055 M) | Ag(s) Consider the cell notation of a galvanic cell given above and the following reduction potentials: Sn- (aq) + 2e- → Sn(s) E° = -0.14 V Ag (aq) + e- → Agis) ED=0.80 V 1. The number of electron transferred in the net reaction is [Select] 2. The E is [Select] 3. The value for Q is (Select] 4. The cell potential for the cell is [Select] V.

Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative

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 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =

Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V

Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V

Given the following two half-reactions, write the overall reaction in the direction in which it is product- favored, and calculate the standard cell potential. Pb2*(aq) + 2 e- - → Pb(s) E° = -0.126 V Fe3*(aq) + e¯ → Fe2*(s) E° = +0.771 V Pb2*(aq) + 2 Fe²*(s) → Pb(s) + 2 Fe³*(aq); = +0.897 V cell Pb2*(aq) + Fe²*(s) → Pb(s) + Fe³*(aq); E, cell = +0.645 V Pb(s) + 2 Fe³*(aq) → Pb²*(aq) + 2 Fe²*(s); F° cell = +1.416 V Pb(s) + 2 Fe*(aq) → Pb²*(aq) + 2 Fe²*(s); E. 'cell = +0.897 V Pb(s) + Fe³*(aq) → Pb²*(aq) + Fe²*(s); = +0.645 V