u Calculate the standard cell potential for each reaction below, andnote whether the reaction is spontaneous under standard state conditions.
1.
Mn(s)+Sn(NO3)2(aq)⟶Mn(NO3)2(aq)+Sn(s)
2.
Na(s)+LiNO3(aq)⟶NaNO3(aq)+Li(s)
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3. Mg(?)+Ni2+(??)⟶Mg2+(??)+Ni(?)
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u Calculate the standard cell potential for each reaction below, andnote whether the reaction is spontaneous under stand...
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)
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 cell potential for the reaction as written at 25.00 °C, given that [Mg2 +] = 0.848 M and [Ni2+] = 0.0110 M. Use the standard reduction potentials in this table. Mg(s) + Ni2+(aq) = Mg2+ (aq) + Ni(s)
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2+] = 0.893 M and [Ni2+] = 0.0140 M. Use the standard reduction potentials in this table. Mg(s) + Ni2+ (aq) = Mg2+ (aq) + Ni(s) E = V
Calculate the cell potential for the reaction as written at 25.00 °C , given that [Mg2+]=0.754 M[Mg2+]=0.754 M and [Ni2+]=0.0200 M[Ni2+]=0.0200 M. Use the standard reduction potentials. Mg(s)+Ni2+(aq) <-- double arrows --> Mg2+(aq)+Ni(s) What is E (in V)?
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
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 Answer Bank Au + (aq) + 3 Ag(s) Au(s) + 3 Ag* (aq) 1,(s) + Cu() — 21(aq) + Cu2+ (aq) Ni2+ (aq) + Pb(s) Ni(s) + Pb2+ (aq)
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
stion 6 of 16 Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2+] = 0.754 M and [Sn²+1 = 0.0190 M. Use the standard reduction potentials in this table. Mg(s) + Sn2+ (aq) = Mg²+ (aq) + Sn(s)
Problem 2. Determine if the following reaction is spontaneous under standard conditions. (more than 2 reactions may be required) Ni(s) + 2 Ce4+(aq) → Ni2+(aq) + 2 Ce3+(aq)