A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential Exed half-reaction 2 H2O(1)+2e → H2(g)+2OH (aq) Ε red -0.83 V 2+ Zn(aq)+2e →>> Zn(s) E = = -0.763 V 'red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. 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. Do you have enough information to calculate the cell voltage under standard conditions? ☐ ☐ ☐ о Yes O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 1 significant digit. Ov ローロ е

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?

Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and I₂ (s), when the two are brought in contact via standard half-cells in a voltaic cell. I2 (s) + 2e → 21¯ (aq) Eº = 0.535 V red Co²+ (aq) + 2e → Co(s) Ee = -0.280 V red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + +

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn"(aq)+2e Zn(s) E=-0.763 V "red MnO,(s)+4H (aq)+2e¯ - Mn²"(aq)+2H,0m E=+1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that U happens at the cathode. O OP 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. Do you have enough information to calculate the cell voltage under standard conditions? Yes O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 3 significant digits.