Determine the spontaneous reaction among these sets of reactants in aqueous solution and write down the...
3) Given: Sn(NO:)2 (aq) + Ni(s) > Sn (s)+ Ni(NO3)2 (aq) Write the standard electrochemical line notation and sketch a complete cell diagram for this electrochemical cell. Calculate the value of E cell.
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as written). Identify each oxidizing agent and reducing agent. Ni (s) + Zn2+(aq) ----> Ni2+(aq) + Zn (s) Ni (s) + Pb2+(aq) -------> Ni2+(aq) + Pb (s) Al (s) + 3 Ag+(aq) ---------> Al3+(aq) + Ag (s) Pb (s) + Mn2+(aq) ----------> Pb2+(aq) + Mn (s)
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.
Determine which of the following pairs of reactants will result in a spontaneous Pb2+(aq) + 2 e- - Pb(s) Eº = -0.13 V Cu+(aq) + e- - Cu(s) E = 0.52 V Ag+ (aq) + e Ag(s) Eº = 0.80 V Br2(+2 e 2 Br-(s) E° = 1.09 V reaction at 25°C. Li+(aq) + e- - Li(s) E° = -3.04 V A13+(aq) + 3 e- → Al(s) E° = -1.66 V Fe3+(aq) + 3 e" -> Fe(s) E° = -0.036...
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.
help with these please Write the cell notation for an electrochemical cell consisting of an anode where Al () is oxidized to AP+ (aq) and a cathode where Pb2+ (aq) is reduced to Pb (s). Assume all aqueous solutions have a concentration of 1 mol/L. Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized to Sn2+ (aq) and a cathode where H(aq) is reduced to H2 (g) at a platinum electrode. Assume...
One electrode of a spontaneous electrochemical cell contains a piece of lead metal dipped into saturated solution of PBSO4 in 1.00 M SO4. The other electrode is a standard hydrogen gas electrode. a) Draw and label all aspects of the electrochemical cell. b) Write the half reactions and the overall electrochemical reaction. c) Determine the emf (Ecell ) for the cell. 1.7 x 10% Ksp PbSO4 Pb (aq) 2 e Note: 2+ E -0.13 V Pb (s)
Need help with questions 1-5 D Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca2+(aq) + Zn(s)-Ca(s) + Zr"(al) (b) 2 Ag+(aq) + Ni(s)--2 Ag(s) + N产(aq) (c) Fe(s) +Mn2 (aą)- Fe (aą)Mn(s) (d) 2 Al(s) + 3 Pb2+(aq) → 2 AP"(aq) + 3 Pb(s) Suppose you wanted to cause Pb ions to come out of solu- tion as solid Pb. What metal could you use to accomplish this? Make a sketch of an electrochemical...
Given which of the following sets of thermodynamic parameters is a reaction spontaneous only at higher temperatures? A) ΔH < 0 and ΔS < 0 B) ΔH < 0 and ΔS > 0 C) ΔH > 0 and ΔS > 0 D) ΔH > 0 and ΔS < 0 ---------------------------------------------------------------------------------------------------------------------------- A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution and a silver electrode immersed in a 1.0 M Ag+ solution. What is the...
i need help answering these qoustions plz?????? Based on the solubility rules given in class, classify the following compounds as solid (s) or aqueous (aq) when added to water: a) Al(OH)3 b) Li3PO4 c) BaSO4 d) (NH4)2CO3 c) Mg(ClO3)2 f) HgCl2 Which combination of reactants results in an acid/base neutralization reaction? a. HNO3(aq) + Zn(s) → b. Mg(C104)2(aq) + NaOH(aq) → c. Ca(s) + H2SO4(aq) - d. H2CO3(aq) + LiOH(aq) → CA OB C What is the net ionic equation...