The reaction is spontaneous when ∆G has a negative value, now ∆G = -nFE
So when E is positive then ∆G is negative and reaction is spontaneous.
The following reactions are shown below to be spontaneous or non spontaneous
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or...
Based on the sign of the standard cell potential, Eco, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Spontaneous as written Nonspontaneous as written Au + (aq) + 3 Ag(s) + Au(s) + 3 Ag+ (aq) Ni²+ (aq) +52- (aq) Ni(s) +S(s) Pb2+ (aq) + H, (g) → Pb(s) + 2 H+ (aq) Answer Bank
thank you for your help! Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Au (aq) + 3 Ag() — Au(s) + 3 Ag+ (aq) 1,(s) + Cu(s) -21"(aq) + Cu+ (aq) Zn2+ (aq) + Sn(s) - Zn(s) + Snº+ (aq) Answer Bank Incorrect Arrange these species by their ability to act as...
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)
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Based on the sign of E cell classify these reactions as spontaneous or nonspontaneous as written assume standard conditions Based on the sign of E degree_cell, classify these reactions as spontaneous or non spontaneous as written. Assume standard conditions.
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s) Fe2+(aq) Pt2+(aq) + Fe(s) Fe2+0.0050 M Pt2+10.035 M The cell is E = V not spontaneous O spontaneous. Cu(s)2 Ag(aq) Cu2t(aq) + 2 Ag(s) [Cu2+0.015 M [Ag 0.015 M The cell is E = V O spontaneous. O not spontaneous Co2+(aq)Ti3(aq)Co3t(aq) +...
Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E ). Pt(s) + Fe2+ (aq) = P22+ (aq) + Fe(s) [Fe2+] = 0.0017 M [P12+] = 0.040 M The cell is O spontaneous. O not spontaneous Cu(s) + 2 Ag+ (aq) = Cu2+(aq) + 2 Ag(s) [Cu2+] =...
12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction written, under standard conditions at 25°C? Eºcell = Eºcathode -Eanode a. Zn2+(aq) + 2Fe2+(aq) → Zn(s) + 2Fe+(aq) b. Ni2+(aq) + Pd(s) - Ni(s) + Pd" (aq)
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...