E° and the Equilibrium Constant 2.) Example: Calculate the equilibrium constant (K) for the following reaction: Ag(S,03), + Fe(CN),+ Ag(s) + 2S,0,2 + Fe(CN),

Q: 5. For the following reaction at 25 °C, 5FE2+ *(aq) + MnO4 (aq) + 8H"(aq) = 5Fe*(aq) + Mn²*(aq) +…

A: Given :  [Fe+2] = 0.50 M  [Fe+3] = 0.10 M  [MnO4-] = 0.025 M  [Mn+2] = 0.015 M pH = 7.00  => [H+]…

Q: 9. At 25° C: AG° is 21.3 kJ for the reaction HCO,H(aq) - H*(aq) + HCO2 (aq) Given that R= 8.314…

A:

Q: Calculate E°cell. Mn(s) + Fe2+(s) (aq) ↔ Mn2+ (aq) + Fe (s) a)E°cell =  ?V  b) Calculate E° for…

A: a) Eocell = Eored cathode - Eored anode  Here cathode: Fe2+ (aq) / Fe (s) Therefore, Eored cathode =…

Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

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Q: To what pH should you adjust a standard hydrogen electrode toachieve an electrode potential of…

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Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

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Q: Calculate AG and K at 25°C for the reactions. a. 7H₂O + 2 Cr³+ + 3 Cl₂ ⇒ Cr₂O7²- + 6 Cl¯ + 14H+ εº…

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Q: What is the pH of the solution in the cathode half-cell when PH2 = 1.0 atm, 3Zn2+4 in the anode…

A: The anodic half-reaction and cathodic half-reaction that occurred in the electrochemical cell are as…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The call reaction at anode is, H2(g) ------> 2H+(aq) + 2e- Standerd cell potential of the cell =…

Q: How many seconds are required to deposit 0.268 grams of iron metal from a solution that contains…

A: Given  Mass deposited (m) = 0.268 g Current (i) = 1.22 A Time (t) = ? S The equation is Fe2+ + 2e-…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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Q: 40. In a galvanic cell, the cathode consists of a Ag"(1.00 M)|Ag half-cell. The anode is a platinum…

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Q: Calculate the cell potential for the galvanic cell in which the reaction   Ti(s)+Co2+(aq)↽−−⇀…

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Q: Co 00 salts are often sparingly soluble, but Co () salts are very, very sparingly soluble. The K of…

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Q: Predict whether the following reactions will be spontaneousin acidic solution under standard…

A: When Gibb's free energy of a reaction delta G is negative, then the reaction is spontaneous. When…

Q: In galvanic cells, the following must be followed to have a spontaneous reaction between Mg and Fe,…

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Q: If at 25°C the standard electrode potential of the Ag/Ag* electrode is 0.799 V, and the equilibrium…

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Q: How long will it take to deposit 1.5 g of Cu on a metal when a current of 5 A is applied to a CuSO4…

A: Given- Amount of copper = 1.5 gMetal of interest = CuCurrent = 5 A To find- Time required

Q: Calculate the cell potential for the galvanic cell in which the reaction. Ti(s)+Cu2+(aq)↽−−⇀…

A: Given Data:

Q: For each of the following reactions, write a balancedequation, calculate the standard emf, calculate…

A: (a)

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: 5. Followed from the previous question, it was determined that K for the reaction at 25°C between…

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Q: Under standard conditions (250 C, 1.0 atm): i. If Cr metal is immersed in a solution of Zn(NO3)2,…

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Q: How many seconds are required to deposit 0.270 grams of copper metal from a solution that contains…

A: Given weight of deposited copper metal from a solution(w) = 0.270 g  Current applied (I)= 0.828 A =…

Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given: Concentration cell of hydrogen. Temperature = 298 K. Concentration of H+ in cathode = 1.00 M…

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. Wate eb. Calculate the equilibrium…

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Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

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Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E"…

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Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

Q: How many grams of iron metal are plated out when a constant current of 8.50 A is passed through…

A: We have 8.5 A of current, passed for 50 minutes, we have to calculate the mass of iron metal…

Q: A steady current of 3 A is maintained for 10 mins in AgNO3 solution. How much Ag is deposited at the…

A: Given: Current is 3 A. Time is 10 minutes. To find: Mass of Ag on cathode

Q: The standard reduction potential (E°) for the conversion of Cr,0 to Cr* at 25°C in an aqueous…

A: Cr2O7 2- + 14H+ + 6e- ------------------> 2Cr3+  + 7H2O            E0(Cr6+/Cr3+)   = 1.33 V  +6…

Q: A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell…

A: Ag+ (aq) + 0.5 H2 (g) ==> H+(aq) + Ag(s)

Q: What is the standard Gibbs free energy change for the reaction between H2O2(aq) and Mn2+ in acidic…

A:

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A:

Q: 4. Calculate AS°, AH°, AG°, and K for each reaction at 298 K. a. 2NO2(g) = 2NO(g) + 02(g)

A: A) 2 NO2 (g) ==> 2 NO(g) + O2 (g)

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: Voltage can be calculated as follows

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: A 0.1 M aqueous CaCl, solution is electrolyzed by usina inert electrodes. If 1.25 ampere current is…

A: At cathode this reaction is taking place,Ca2+  +  2e-   →  Ca  Calculate the charge first,Q = it and…

Q: Given the following half-reactions and their standard reduction potentials, 2CIO;- + 12H* + 10e Cl,+…

A: E0ClO32- =1.47 V E0S2O82- = 2.01 V E0 cell = E0S2O82-  -E0ClO32-  = 2.01 - 1.47 = 0.54 V

Q: What mass of Fe(s) may be deposited from an aqueous FeCl2 solution if a current of 2.50 A is applied…

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Q: 1. Consider a cell buffered at pH 2.00 and consists of Fe2+(aq) (0.004 M), Fe3+(aq) (0.070 M) and…

A: Redox reactions in electrochemistry are characterized as chemical processes in which electrons…

Q: A steady current of 5 A is maintained for 120 seconds in CUSO4 solution. How much Cu is deposited in…

A: The charge deposited is given by the product of charge and time. Q=It where I is the current and t…

Q: An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 3.00 A passing…

A: Given Current (I) = 3A Given mass = 1.572g Time = 25min = 1500s Molecular weight = 101.07g

Q: Calculate the equilibrium constant, K for the reaction at 298 K,Zn (s) + Cu2+(aq) ——–>  Zn2+(aq)…

A: Equilibrium constant may be defined as the ratio of the multiplication of the concentration of the…

Q: The standard cell potentials for following reaction at standard room temperature are E Fe/Fe =…

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Q: The standard state cell potential for the reaction below is 1.030 V. Zn(s) + Hg,Cl,(s) → ZnCl,(aq) +…

A: Given: Cell potential =E°cell=1.030 V Temperature= 298 K To find: Standard state Gibb's energy…