1.) 2Cl Cl2(g) K = 3.44
x 105
What happens if the concentrations of Cl is 0.045 M and the
concentration of Cl2 is 0.23 M?
2.) We have FeCl2. We can put this into a solution of either 0.1 M Fe(NO3)3 or 0.1 M MgCl2. Which one will result in higher solubility?
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1.) 2Cl Cl2(g) K = 3.44 x 105 What happens if the concentrations of Cl is 0.045...
3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.594 M , [Co2+]= 0.858 M , and [Cl−]= 0.723 M , and the pressure of Cl2 is PCl2= 8.00 atm ?
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 6.60×10−2 M , [Co2+]= 0.684 M , and [Cl−]=0.346 M , and the pressure of Cl2 is PCl2= 3.40 atm ?
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.727 M , [Co2+]= 0.662 M , [Cl−]=0.795 M , and [Cl2]= 0.200 M ? Express your answer with the appropriate units.
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 1.90×10−2M , [Co2+]= 0.510 M , and [Cl−]= 0.289 M , and the pressure of Cl2 is PCl2= 7.80 atm ?
for the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.788 M , [Co2+]= 0.157 M , and [Cl−]= 0.702 M , and the pressure of Cl2 is PCl2= 2.90 atm ? Express your answer with the appropriate units.
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.223 M , [Co2+]= 0.551 M , and [Cl−]= 0.209 M , and the pressure of Cl2 is PCl2= 8.90 atm ? Express your answer with the appropriate units.
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.294 M , [Co2+]= 0.749 M , and [Cl−]= 0.770 M , and the pressure of Cl2 is PCl2= 3.60 atm ? Express your answer with the appropriate units.
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.522 M , [Co2+]= 0.760 M , and [Cl−]= 0.409 M , and the pressure of Cl2 is PCl2= 9.40 atm ? Express your answer with the appropriate units.
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates, as shown below. 2K.[Fe(CN),](aq) +Cl2(g) = 2Ks[Fe(CN)2](3) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C [Fe(CN).J” (aq) + € → [Fe(CN).]" (aq) E = 0.356 V Cl2(g) + 2e → 2Cl(aq) E* = 1.360 V Kup of Kj[Fe(CN).] = 106.5 Answer: b. When 80.0 mL of 1.00 M KCN is added to...