What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 6.29×103 atm, the H* concentration is 1.17M, and the A13+ concentration is 6.41×10-4M? 6H+(aq) + 2Al(s) >>3H2(g) + 2A13+(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Use the standard reduction potentials given below to predict if a reaction will occur when Zn metal is put into a 1 M aqueous Mn2+ solution. Zn2+(aq) + 2eZn(s) E red = == = -0.763 V Mn2+ (aq) + 2eMn(s) E Mn(s) Ed -1.180 V red If a reaction will occur, write a balanced net ionic equation for the reaction. 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.) + +
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 6.29×103 atm, the H* concentration is 1.17M, and the A13+ concentration is 6.41×10-4M? 6H+(aq) + 2Al(s) >>3H2(g) + 2A13+(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Use the standard reduction potentials given below to predict if a reaction will occur when Zn metal is put into a 1 M aqueous Mn2+ solution. Zn2+(aq) + 2eZn(s) E red = == = -0.763 V Mn2+ (aq) + 2eMn(s) E Mn(s) Ed -1.180 V red If a reaction will occur, write a balanced net ionic equation for the reaction. 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.) + +
Chapter19: Applications Of Standard Electrode Potentials
Section: Chapter Questions
Problem 19.8QAP
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