Given the electrochemical cell described by: Mn(s)| Mn2+(aq)||Cr3+ (aq)| Cr(s) Calculate the cell potential at 250C if the concentration of Mn2+ (aq) is 0.800 M and the concentration of Cr3+ (aq) is 0.500 M. Report your answer to 3 significant figures. Use theStandard Reduction Potentials Table as needed. Ecell = V

A galvanic cell is powered by the following redox reaction: 2+ MnO (aq) + 8H(aq) + 5 Cu* (aq) Mn²+ (aq) + 4H₂O(1) + 5 Cu²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. Ov V 0-0 e X

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) + I¯(aq) = 1₂(s) + Cr³+ (aq) ४० spontaneity: (م) spontaneous not spontaneous balanced equation: chemPad XX→ ← (b) Cr₂0₂² (aq) + F¯(aq) = F₂(g) + Cr³+ (aq) 8⁰ V spontaneity: spontaneous not spontaneous balanced equation: chemPad XX Help H₂(g) → H+ (aq) + H(aq) Greek Help Greek

A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution.  The Ecell at 20oC (293K) is measured as +1.03 V. Calculate the experimental standard cell potential, Eocell, for the reaction

Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.24 volts.

Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag               Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr            Eo= -0.74 V

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)

A cell constructed in which one half-cell consists of a Zn wire dipped in a solution of Zn(NO3)2- The other half-cell is composed of an inert electrode in a solution containing a mixture of Fe and Fe* ions. What will the cell potential, Ecell, be if the soluble ions have the following concentrations at 25°C? [Zn**] = 0.49M; [Fe] = 0.16 M; [Fe*] = 0.41 M Draw the complete galvanic cell set-up for this. Label each component.

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!

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