Every answer I've make the efforts so much is wrong and also every answer I have looked up is additionally wrong.

You are watching: Compute the equilibrium constant for the spontaneous reaction between cd2+(aq) and zn(s).

I have one attempt remaining before I lose all credit transaction for the problem.

I went around solving this trouble by calculating the E-cell the Ni2+ and Zn i beg your pardon is E-Cathode - E-Anode i beg your pardon is (-0.23-0.76)=-0.099

I then supplied the Ecell=(0.0592/n)logK formula

Since there room 2 electron involved, n=2

-0.99 = (0.0592/2)logK

K= 3.58 * 10-34

This is wrong.

Other answers I have actually tried: 1.7 * 1017 , 1.8 * 1017 , and

2.0 8 1017

I have no proviso what ns am law wrong. Ns literally just plugging stuff into the formula. I even looked increase the answer and that to be wrong too.

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level 1
· 4 yr. Ago
Your consumption of the formula is correct however you have actually not calculate the voltage properly:

Let's compose out the fifty percent reactions.

Ni2+ (aq) + 2e- -> Ni (s)

Zn (s) -> Zn2+ (aq) + 2e-

The palliation potential that the pair Ni2+/Ni is -0.23V.

The palliation potential the the pair Zn2+/Zn is -0.76. However, this is reduction. In this electrochemical cell, zinc is being oxidised. Therefore the potential the the pair Zn/Zn2+ is 0.76V.

When you add the voltages of the half reactions you gain a voltage for the as whole reaction that 0.53V. The remainder of the inquiry you did correctly, but since you had the voltage not correct it came out wrong.

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level 1
· 4 yr. Ago

You're never ever going to gain a negative cell voltage.

See more: Oogle How Many Days Since June 12 1829 Joke, The Parliamentary Debates

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