Cu2+(aq) + Au(s) Cu+(aq) + Au+(aq) A student studying the reaction represented above constructs a v…

Cu2+(aq) + Au(s) Cu+(aq) + Au+(aq) A student studying the reaction represented above constructs a voltaic cell as shown in the diagram below. The cell contains an Au(s) electrode in 0.0 M Au(NO3)2(aq) and a Cu(s) electrode in a beaker containing 0.0 M CuNO3(aq) and 0.0 M Cu(NO3)2(aq). Voltmeter Cu(s) | Cu2+(aq) || Au+(aq) | Au(s) The standard reduction potentials associated with the cell are given in the following table: Half-reaction E° (V) Cu2+(aq) + 2e- - gt; Cu(s) 0.16 Au+(aq) + e- - gt; Au(s) 1.50 Calculate the value of the standard cell potential, E°. Does the mass of the Cu(s) electrode increase, decrease, or remain the same as the cell operates? Justify your answer.

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