A Zn2+ l Zn half-cell is connected to a Cu2+ l Cu half-cell tomake a galvanic ce

Question

A Zn2+ l Zn half-cell is connected to a Cu2+ l Cu half-cell tomake a galvanic cell, ( l = salt bridge stuffs) inwhich Zn2+=Cu2+=1.00M. The cell voltage at 25 degrees ismeasured to be E=1.3V, and Cu is observed to plateout as the reaction proceeds. Calculate G for the chemical reaction thattakes place in the cell, for 1.00mol of zinc dissolved. I know what and how to solve the problem once I get equations.However, I'm not sure what to start with. (E.g. How do I knowif I have to start with Zn2+ Zn or Zn Zn 2+?) Andthe salt bridge equation or something (Zn2+ l Zn) doesn't eaxactlytell me anything. What does "PLATE OUT" mean? Does that give ahint?  I do not need algebraic solution to thisquestion. I really want to know how I'm supposed to figure out "HOWTO START EQUATIONS." A Zn2+ l Zn half-cell is connected to a Cu2+ l Cu half-cell tomake a galvanic cell, ( l = salt bridge stuffs) inwhich Zn2+=Cu2+=1.00M. The cell voltage at 25 degrees ismeasured to be E=1.3V, and Cu is observed to plateout as the reaction proceeds. Calculate G for the chemical reaction thattakes place in the cell, for 1.00mol of zinc dissolved. I know what and how to solve the problem once I get equations.However, I'm not sure what to start with. (E.g. How do I knowif I have to start with Zn2+ Zn or Zn Zn 2+?) Andthe salt bridge equation or something (Zn2+ l Zn) doesn't eaxactlytell me anything. What does "PLATE OUT" mean? Does that give ahint?  I do not need algebraic solution to thisquestion. I really want to know how I'm supposed to figure out "HOWTO START EQUATIONS."

Explanation / Answer

We know that:

     In the electrochemical series Zn ismore reactive than Cu as per their standard reductionpotentials.

      Oxidation half reaction:

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