Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Pt Cr 0.10 M MnO4 0.40 M Cr+ 0.20 M Mn2+ 0.30 М Сr,0,2 0.010 M H* 0.010 MH* The standard reduction potentials are as follows: MnO4+ 8H* + 5e Cr20,2-+ 14H* + 6e¯ - Mn2+ + 4H,O, ɛ° = 1.51 V 2Cr* + 7H2O, ɛ° = 1.33 V What is the cell potential at 25°C as read on the digital voltmeter? 0.18 V 2.58 V 0.10 V 0.59 V O 0.26 V

Consider a galvanic electrochemical cell constructed using Cr/Cr* and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: Crs* (aq) + 3 e Cr(s) E°red = -0.744 V Zn2*(aq) + 2 e Zn(s) E°red = -0.763 V What is the standard cell potential for this cell?

== A certain half-reaction has a standard reduction potential E red - 1.32 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be…

Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: 3+ Cr**(aq) + 3 e → Cr(s) E°red = -0.744 V Zn2*(aq) + 2 e → Zn(s) E°red = -0.763 V What is the cell potential for this cell at 25 °C when [Zn2*] = 0.0323 M and [Cr3] = 0.1736 M?