Consider the following equation: Fe2O3(aq)  +  3CO(g)    →   2Fe(s)  +  3CO2(g) Identify the species (element or ion) that is acting as the oxidizing agent

Calculate the Ecell for the following reaction? Zn(s)  +  Fe2+(aq, 0.1 M)  ↔  Zn2+(aq, 1.9 M)  +  Fe(s) Use:  Zn2+(aq)  +  2e-  ↔  Zn(s)  Ecell = -0.76 V Fe2+(aq)  = 2e-  ↔  Fe(s)  Ecell = -0.447 V

A Ni-Cd battery powers electrical devices through the following reaction Cd(s)  +  NiO2(s)  +  2H2O(l)    →    Cd(OH)2(s)  +  Ni(OH)2(s) Identify the species (element or ion) that is getting reduced

Identify the correct statement for following reaction Zn(s)+  2Na+(aq) → Zn2+(aq)  +  2Na(s) Use: Zn2+(aq)  +  2e-  =  Zn(s)    Ecell = -0.76 V Na+(aq)  +  e-  =  Na(s)  Ecell = -2.71 V

Based on the Gibbs free energy you received for question (25), calculate the equilibrium constant for the reaction. Use ΔG = -RT ln K: Temperature 25 Celsius, R = 8.314 J / mol. K

The conditions necessary for a SHE is

Lewis acidity of a metal ion generally increases with

Using the following two half-cells, design a spontaneous reaction and find its cell voltage Al3+(aq)  +  3e-  ↔  Al(s)            Ecell = -1.676 V Sn4+(aq)  +  2e-  ↔  Sn2+(aq)  Ecell = 0.154 v

Which of the following is most likely to act as a Lewis acid?

An electrochemical cell has been built by using the following two half cells SO42-(aq)  2e-  +  4H+(aq)  →  SO2(g)  +  2H2O   Ecell = 0.21 V K(s)  →   K(s)+(aq)  +  e-     Ecell = -2.92 V Identify the complete cell reaction