Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) |...
Hi can someone help me with these questions, Thank you: Question 8 (1 point) The standard potential of the cell Ni(s) Ni2+(aq) || Cl(aq) AgCl(s) Ag(s) is +0.45 V at 25°C. If the standard reduction potential of the AgCl|Ag|Ci couple is +0.22 V, calculate the standard reduction potential of the Ni2+INi couple. -0.45 V +0.23 V -0.67 v +0.67 v 0 -0.23 V Question 6 (1 point) The standard reduction potential of the Br2/Brand Sna/Sn couples are +1.07 and -0.14...
Question 6 (1 point) Saved The standard potential of the cell In(s) | In3+ (aq) || Cu2+(aq) | Cu(s) is +0.68 V at 25°C. If the standard reduction potential of the Cu2+1Cu couple is +0.34 V, calculate the standard reduction potential of the In3+|In couple. O +1.02 V © -0.34 v 0 -0.23 V 0 +0.34 V 0-0.68 V
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
In the following cell, A is a standard Sn2+Sn electrode connected to a standard hydrogen electrode. If the voltmeter reading is -0.14 V, match each electrode with its correct name. Given: Standard reduction potential of the Ht/H2 and Sn2+/Sn couples are 0.00 and -0.14 V, respectively. Hy (9) standard hydrogen electrode 1. anode Sn2+ Sn electrode 2. cathode
Question 5 (1 point) Given: Cr3+(aq) + 3e --> Cr(s); E° = -0.74 V Sn2+(aq) + 2e- --> Sn(s); E° = -0.14 V What is the standard cell potential for the following reaction? 2Cr(s) + 3Sn2+(aq) --> 3Sn(s) + 2Cr3+(aq)? 0-0.60 v 0 +0.60 v O +1.06 V 0 +0.88 V 0-0.88 V
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) II Ag+(aq, 0.55 M)1 Ag(s) Sn2+ (aq) + 2 e Ag+ (aq) + e- Sn(s) Ag(s) E = -0.14 V E = 0.80 V -0.84 V +0.86 V 0 -0.93 V +1.12 V O 0.92 V
1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). A. If the concentration of Sn2+ in the cathode compartment is 1.30 M and the cell generates an emf of 0.25 V , what is the concentration of Pb2+ in the anode compartment? B. If the anode compartment contains [SO2−4]= 1.30 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4? 2. A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). A. What is the emf...
A voltaic cell employs the following redox reaction: Sn2+(aq)+Mn(s)---- Sn(s)+Mn2+(aq) Calculate the cell potential of 25 degrees Celsius under each of the following conditions. Part A: Sn2+= 1.15*10^-2 M; and Mn2+= 2.37 M Part B: Sn2+= 2.37 M; and Mn2+= 1.15*10^-2
The calculated cell potential for the Sn(s) + Br2(l) → 2 Br- (aq) + Sn2+(aq) cell is?
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s) E = +0.80 V Sn2+ (aq) + 2 e Sn(s) E = -0.14 V Identify the anode and give the cell voltage under standard conditions: O A Sn: Eºcell = -0.66 V B. Sn; Eºcell = 0.66 V O C. Ag: Eºcell = 0.67 V D. Ag: Eºcell = 0.94 V E. Sn; Eºcell = 0.94 V