An electrochemical cell consists of a standard hydrogen electrode and a copper m

Question

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode.

What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 5.2×10-5 M?

The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.184 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.)

A calibration curve to show how the cell potential varies with [Cu2+] may be constructed. A plot of cell potential (in V, with the same sense as in question 1) versus log10[Cu2+] should yield a straight line. What is the slope of this line?

Explanation / Answer

Since y=mx+c and you said y=E and x=log(Cu2+) reduced, relate that to the linear equation:
Slope is just what n is.
Y= mx + c
E=(0.0592/n)log([Cu2+]) + E0

so the n corresponds to the m, or the slope of the equation.

What is n?

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