Question

Constants

The following values may be useful when solving this tutorial.

Constant	Value
E∘Cu	0.337 V
E∘Ni	-0.257 V
R	8.314 J⋅mol−1⋅K−1
F	96,485 C/mol
T	298 K

Part A

In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are

Cu2+(aq)+2e−→Cu(s)

and

Ni(s)→Ni2+(aq)+2e−

The net reaction is

Cu2+(aq)+Ni(s)→Cu(s)+Ni2+(aq)

Use the given standard reduction potentials in your calculation as appropriate.

Express your answer numerically to three significant figures.

Keq= __________?

please help solve for Keq - i will rate! :)

Answer 1

u)= CuA) 0.337 NiA) E 0.257 V ut ulA)t Ni E 0.337 t 0.257 0.594 D4-MFE RTnKeg ne2,2 ox olve jin the readio) -2X96495X0-594 - -9-314299x keg Kerz 124 Xlo20

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