Question

Part A Describe the electrodes in this nickel-copper galvanic cell. Drag the appropriate items to their respective bins. View Available Hint(s) ResetHelp Nickel Copper Standard reduction potentials for nickel(II) and copper(II) The standard reduction potential for a substance indicates how readily that substance gains electrons relative to other substances at standard conditions. The more positive the reduction potential, the more easily the substance gains electrons. Consider the following: Ni2+(aq)+2e−→Ni(s),Cu2+(aq)+2e−→Cu(s), E∘red=−0.230 V E∘red=+0.337 V Part B What is the standard potential, E∘cell, for this galvanic cell? Use the given standard reduction potentials in your calculation as appropriate.

Answer 1

Answer:

Part-A:

Anode is Nickel and Cathode is copper.

Part -B:

$E^{0}_{cell}$ of the reaction is 0.567V.

Explanation:

Nickel-Copper cell electrodes are "Ni" and "Cu" rod.

Nickel electrode is dipped in $Ni^{+2}$ solution.

Copper electrode dipped in $Cu^{+2}$ solution.

Part -A:

Anode:

At anode oxidation takes place

$Ni(s) \rightarrow Ni^{+2}(aq)+2e^{-}$

Hence, anode is Nickel.

Cathode:

At cathode reduction takes place.

$Cu^{+2}+2e^{-} \rightarrow Cu(s)$

Hence, Cathode is copper.

Part-B:

$E^{0}_{cell}=E^{0}_{cathode}-E^{0}_{anode}$

$=0.337-(-0.230)=0.567V$

Hence, $E^{0}_{cell}$ of the reaction is 0.567V.

Answer 2

Anodes and cathodes are the electrodes where oxidation and reduction take place.

What are the electrodes in galvanic cell?

Electrochemical cells have two electrodes which is called anode and cathode. The anode is the electrode where oxidation occurs while the other hand, cathode is the electrode where reduction takes place so we can conclude that anodes and cathodes are the electrodes where oxidation and reduction take place.

Learn more about electrodes here: https://brainly.com/question/18251415