What minimum concentration of Sn2+ would be necessary to make the following reaction spontaneous at 25°C if [Pb2+] = 1.0 M?
Pb(s) + Sn2+(aq) → Pb2+(aq) + Sn(s)
1.5 M
2.2 M
0.68 M
1.1 M
0.46 M
What minimum concentration of Sn2+ would be necessary to make the following reaction spontaneous at 25°C...
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 1.50 M and the cell generates an emf of 0.22 V , what is the concentration of Pb2+ in the anode compartment? b. If the anode compartment contains [SO2−4]= 1.50 M in equilibrium with PbSO4(s), what is the Kspof PbSO4?
The free energy change for the following reaction at 25°C, when [Fe2+1 = 8.61*10' M and (Sn2t - 1.17 M. is 70.1 kJ Fe2+(8.61x10 3 M) + Sn(s) Fe(s) + Sn2+(1.17 M) AG = 70.1 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction? Submit Answer Retry Entire Group 3 more group attempts remaining The free energy change for the following reaction...
The free energy change for the following reaction at 25°C, when [Sn2+] = 1.18 M and [Fe2+] = 4.88 10-M.is -71.5 kJ: Sn2+(1.18 M) + Fe(s)— Sn(s) + Fe2+(4.88 10-3M) AG = -71.5 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction?
The free energy change for the following reaction at 25 °C, when (Sn2+] = 3.22x10-M and [H]=1.13 M, is 41.6 kJ: Sn2+(3.22x10-9 M) + H2(g)—Sn(s) + 2H+(1.13 M) AG - 41.6 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Question 30 (6 points) What is the equilibrium constant (K) at 25°C for the following cell reaction? Sn(s) + Pb2+ (aq) → Sn2+ (aq) + Pb(s); Eºcell = 0.014 V (Please submit your detail solution work to the dropbox, which can be found in the assignments.) A/
5. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf Eº of an electrochemical cell described by the following reaction: Pb + Sn2+ --> Pb2+ + Sn (b) What is the value of E if the concentration of Sn is 1.26 x 10-2 and the concentration of Pb2+ is 7.11 x 10-5? (c) If E = 0.16 V and Sn2+ = 0.10 M, what is the concentration...
Determine what redox reaction, if any, occurs (at 25°C) when tin metal (Sn) is added to (a) a 1.0 M solution of NiCl, and (b) a 1.0 M solution of HCl. (a) Sn is added to a 1.0 M solution of NiCl2 o o O O Sn(s) + Ni2+(aq) → Sn2+(aq) + Ni(s) Sn2+(aq) + 2C1(aq) → Sn(s) + Cl2(8) Ni2+(aq) + 2CI+ (aq) → Ni(s) + Cl2@) No reaction. (b) Sn is added to a 1.0 M solution of...
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Fe3+(aq) +Al(s) Pb2+(aq) + Au(s) Na+(aq) + Cr(s) Ag+(aq) + Br−(aq) None of the above pairs will react.
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Pb2+(aq) + Ag(s) Fe3+(aq) +Cd(s) Ag+(aq) + Br-(aq) Li+(aq) + Al(s) None of the above pairs will react.
Question 1) What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Pb(s) and Sn2+(aq) to give Sn(s) and Pb2+(aq) Use the reduction potential values for Sn2+(aq) of -0.14 V and for Pb2+(aq) of -0.13 V Question 2) What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: Cr(s) and Cu2+(aq) to give Cu(s) and Cr3+(aq) Use the reduction potentials for Cr3+(aq) is -0.74 V and...