Consider the data in the table below and an electrochemical cell where the follo
ID: 1068981 • Letter: C
Question
Consider the data in the table below and an electrochemical cell where the following unbalanced chemical reaction takes place: _Au^1+ [aq] + _zu[s] rightarrow _Au[s] + zn^2+ [aq] How many total electrons are transferred in this redox reaction? 4 3 2 1 Which of the following represents the correct line notation for this cell? Au(s) | Au^1+ (aq)|| Zn^2+ (aq)| Zn(s) Au^1+ (aq)| Au(s)|| Zn(s)| Zn^2+ (aq) Zn^2+ (aq)| Zn(s)||Au(s)| Zu^1+ (aq) Zn(s)| Au^1+ (aq)|| Zu^2+ (aq)| Au(s) Zn(s)| Zn^2+ (aq)|| Au^1+(aq)| Au(s) If the cell voltage under standard conditions (E^cell) = 2.44 V, what is the standard reduction potential for the reduction of Au^+1? 1.68 V -1.68 V +3.2 V -3.2 V Which of the following statements about this cell are correct? The reaction is spontaneous because delta G degree = -235 kJ The reaction is spontaneous because delta G degree = -471 kJ The reaction is non-spontaneous because delta G degree = -471 kJ The reaction is non-spontaneous because delta G degree = -235 kJ What will a voltmeter read, if you operate the cell at 40 degree C using a 0.031 M AuNO_3 solution and a 0.28 M Zn(NO_3)_2 solution? 2.52 V 2.46 V 2.44 2.41 V 2.36 V Now consider only the gold half-cell. How many grams of gold could be plated out of the solution if a current of 0.5 Amps is passed through a 1.19 M AuNO_3 solution for 30 minutes? 17.9 g 3.67 g 2.38 g 1.84 gExplanation / Answer
5)
oxidation numbers
çAu = +1
Zn = +2
so
1x2 = 2 electrons must be being transferred
c)
Au will reduce, since it goes from +1 to 0
this goes in the right side cell notation
so
Zn(s) / Zn+2(aq) // Au+(aq) / Au(s)
Q7
Ecell = Ered - Eox
2.44 = Egold- (-0.76)
Egold = 2.44- 0.76 = 1.68 V
Q8
Apply:
dG = -nFEªcell
dG = -2*96500*2.44 = -470,920 J = -470.920 kJ/
this must be spotanous, since dG is negative
Consider posting multiple questions in multiple set of Q&A. We are not allowed to answer to multiple questions in a single set of Q&A