A student makes a concentration cell with two Cu electrodes using 1.0 M CuSO_4 and 0.01 M CuSO_4....
Question:
A student makes a concentration cell with two {eq}Cu {/eq} electrodes using 1.0 M {eq}CuSO_4 {/eq} and 0.01 M {eq}CuSO_4 {/eq}.
A. Calculate {eq}E_{cell} {/eq} for this concentration cell.
B. Would {eq}E_{cell} {/eq} be different if {eq}Ag {/eq} electrodes and 1.0 M {eq}AgNO_3 {/eq} and 0.01 M {eq}AgNO_3 {/eq} were used? Explain.
Nernst Equation:
The cell potential of an electrochemical (redox) reaction system varies with its chosen set of conditions. This includes the molarity values of redox-active species dissolved inside an aqueous solution. A standard cell potential has 1.0 M for all of these molarity values. Any deviation from these values results in a non-standard cell potential that deviates from the standard value. This deviation is described through the Nernst equation. A reaction quotient "Q" term is present that is constructed from the balanced stoichiometry of the non-standard species. Their molarity values are inserted into the "Q" expression and the resulting value is {eq}\rm Q \neq 1 {/eq}.
Answer and Explanation: 1
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A concentration cell is a type of voltaic cell with identical half-cell chemistry. Therefore, by definition its standard cell potential...
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