from data table:
Eo(Sn2+/Sn(s)) = -0.14 V
Eo(Cl2(g)/2Cl-) = 1.36 V
As per given reaction/cell notation,
cathode is (Cl2(g)/2Cl-)
anode is (Sn2+/Sn(s))
Eocell = Eocathode - Eoanode
= (1.36) - (-0.14)
= 1.50 V
here, number of electrons being transferred, n = 2
Eo = (2.303*R*T)/(n*F) log Kc
At 25 oC or 298 K, R*T/F = 0.0592
So, Eo = (0.0592/n)*log Kc
1.5 = (0.0592/2)*log Kc
log Kc = 50.6757
Kc = 4.739*10^50
Answer: 4.7*10^50
Use the data in the table below to calculate the equilibrium constant at 25°C for the reaction: Cl2(g) + Sn(aq) + Sn2+...
Calculate the equilibrium constant for each of the reactions at 25 ∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Pb2+(aq)+2e− →Pb(s) -0.13 Zn2+(aq)+2e− →Zn(s) -0.76 Br2(l)+2e− →2Br−(aq) 1.09 Cl2(g)+2e− →2Cl−(aq) 1.36 MnO2(s)+4H+(aq)+2e− →Mn2+(aq)+2H2O(l) 1.21 Pb2+(aq)+2e− →Pb(s) -0.13 Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) Express your answer using two significant figures.
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Sn2(aq) + 21'(aq) —Sn(s) +12() Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be than zero
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Sn2 (aq)+2Fe2 (aq) Sn(s)+2Fe (aq) e3+ Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: than zero. AG° for this reaction would be
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) + Sn(s) = 2Ag(s) + Sn2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: G° for this reaction would be (greater/less) than zero.
Calculate the equilibrium constant for each of the reactions at 25∘C∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction Cl2(g)+2e ---> 2CI- 1.36 I2(s)+2e --> 2I- 0.54 Part A Cl2(g)+2I−(aq)→2Cl−(aq)+I2(s) K= ?
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cr (aq)+Sn(s)2 Cr (aq) + Sn2 (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant than zero. AGo for this reaction would be
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
11A. 11B. 11C. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Sn2+(aq) + 2Fe2+(aq)— Sn(s) + 2Fe3+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would bv _ than zero. greater less Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cuºt(aq) + Co(s) + Cu(s) + Coºt(aq) Hint: Carry at least 5 significant figures during...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cr}*(aq) + Sn(s)—2Cr?*(aq) + Sn²+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be than zero.
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...