1. Calculate the standard cell potential cell that uses the Mg/Mg2+ and Cu/Cu* half- cell reactions...
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...
Be sure to answer all parts. Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reaction at 25°C. E______ = V Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cu²+ (aq)+e. → Cut (aq) En e = +0.153 V NO3(aq)+41 (aq)+3 → NO(g)+2H 0(1) Ered = +0.96 V 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. x 6 ? Write a balanced equation for the overall reaction that powers the cell....
Calculate the equilibrium constant of a cell that uses a Mg/Mg2+ half-cell and a Cu/Cu2+ half-cell.
Calculate the standard emf of a cell that uses Ag/ Ag and Al/A13+ half-cell reactions. Write the cell reaction that occurs under standard-state conditions. 18.12
Be sure to answer all parts. A galvanic cell using Mg / Mg2+ and Cu Cu half-cells operates under standard-state conditions at 25 oC, and each compartment has a volume of 228 mL. The cell delivers 0.28 A for 31.0 h. (a) How many grams of Cu are deposited? g Cu (b) What is the [Cu2+ remaining? Be sure to answer all parts. A galvanic cell using Mg / Mg2+ and Cu Cu half-cells operates under standard-state conditions at 25...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn(s) red -0.763 V Zn2+ (aq)+2e NO3(aq)+4 H+ (aq)+3e NO(9)+2H20(1) EO red = +0.96 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. е х 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...
A chem igns a galvanic cell that uses these two half reactions: standard reduction potential half-reaction (aq)+4 H,0(1)+3e" → Cr(OH)2(3)+50H (aq) cro Ered=-0.13 V Fe?+ (aq)+e → Fe2+ (aq) E = +0.771 V Answer the following questions about this cell. 0-0 0 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. X 5 Write a balanced equation for the overall reaction that powers the cell....
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential = +0.771 V Fe'+ (aq)+e — Fe2+(aq) N2(9)+4 H20(1)+44 → N2H4(aq)+4 OH(aq) Eed=-1.16 V 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....
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction Br2)+2e 2 Br (aq) 1.065 V red E 2 H,00+2е H2(9)+2ОН (ад) 0.83 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...