The standard cell potential of the reaction is 1.10 V for the cell Zn (s)/Zn2+//Cu²+/Cu (s) If the Zinc ions have a concentration of 0.0010 M and the copper (II) ions have a concentration of 1.00 M, calculate the electromotive force (EMF) of the cell. Based on A GO of the cell, the reaction is classified as

Q: ne standard cell potential of the reaction is 1.10 V for the cell in (s)IZn2+//Cu2+/Cu (s) the Zinc…

A: Given E° = 1.10V  [Zn²+]= 0.010M . [Cu²+] = 1.00 M  We have to find EMF of cell and find ∆G° of cell…

Q: The standard cell potential (E° cell) for the reaction below is +1.10 V. The cell potential for this…

A: E°cell = +1.10V [Cu^+2]=1.0×10^-5M [Zn^+2]=3.0M

Q: A cell is composed of a pure copper and pure lead electrode immersed in solutions of their bivalent…

A: Given: Concentration of bivalent copper ion i.e. Cu2+ = 0.3 M Cell potential, Ecell = 0.507 V And…

Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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Q: Consider the following redox reaction: Sn2+  +  Sr(s)  -->  Sn(s)  +  Sr2+ What is the cell…

A: Given, concentrations of Sn2+ and Sr2+ are 3.5M & 0.05M respectively at temperature 10°C. The…

Q: Calculate AG° and K for the following cell reactions. State whether the cell reaction is spontaneous…

A: recall the given reaction and also the values of electrode potential of the given half cell Cus +…

Q: For the reaction : Cu+2(ag) + Sns) →Cu(s) + Sn+2(ag) Cut2(ag) = 0.12 M Snt2 conditions are (ag) =…

A: Given: Concentration of Cu+2(aq)= 0.12 M Concentration of Sn+2(aq) = 0.03 M

Q: An electrochemical cell is constructed such that on one side a pure cadmium electrode is in contact…

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Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

A: The given cell notation is: Cu|Cu2+0.020 M||Cu2+2.0 M|Cu It is a concentration cell (electrolytic…

Q: The cell notation for the Galvanic cell is Cd(syCd2+/l/½(syI" The Standard Reduction Potential are…

A: The Gibb's free energy determines the spontaneity of a reaction. If the Gibb's free energy is…

Q: A cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given :  E°Zn+2/Zn  = -0.76 V  E°Cu+2/Cu = 0.34 V  [CuSO4] = 0.01 M  [ZnSO4] = 0.02 M

Q: The standard reduction potential of Cu(s) is + 0.339 V. What is its standard oxidation potential?…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr*] = 0.810 M and…

A: The cell reaction given is, => Cr (s) + Fe2+ (aq) ⇔ Cr2+ (aq) + Fe (s) Given: [Cr2+ ] = 0.810 M…

Q: The free energy change for the following reaction at 25 °C, when [Pb²+] = 1.20 M and Zn²+ ] =…

A: Recall the given reaction,                              Pb2+ 1.20 M  +  Zn s  →  Pb s  +  Zn2+…

Q: The cell notation for the Galvanic cell is              A(s)/A2+//B2(s)/B- The Standard Reduction…

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Q: O ELECTROCHEMISTRY Understanding concentration cells 1/5 A certain metal M forms a soluble sulfate…

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Q: 7. A galvanic cell at 25°C consists of an electrode of zinc in a 0.10 M ZNSO4 solution and anther of…

A: An electrochemical cell is a type of cell which converts chemical energy into electrical energy.…

Q: The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for…

A: Given,   2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq)   We need to Calculate the following for the…

Q: ) Consider the galvanic cell, Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s). Which one of the following…

A: Galvanic cell : The notation in galvanic cell is written as : So , the reaction for given cell…

Q: The free energy change for the following reaction at 25 °C, when [Ag*] = 1.12 M and [Ni2+] =…

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Q: The cell notation for the Galvanic cell is Cd(s)/Cd2+//I2(s)/I- The Standard…

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Q: The cell notation for the Galvanic cell is              Cd(s)/Cd2+//I2(s)/I- The Standard…

A: Cell notation for the Galvanic cell is :-             Cd(s)/Cd2+//I2(s)/I-

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.20 M and [Pb2+] =…

A: Equilibrium constant can be defined as the ratio of concentration of products to concentration of…

Q: Calculate the cell potential of tho following cell at 25°C. Cr(s) | C" (1.0 X 10° M) || Ni²* (1.5 M)…

A: Given data,[Cr3+]=1.0×10-3M[Ni2+]=1.5MTemperature=25oC

Q: what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The…

A: The solution is as follows :

Q: An electrochemical cell is constructed such that on one side a pure Zn electrode is in contact with…

A: The electrode which has a higher reduction potential has a greater tendency to gain electrons and it…

Q: Consider the galvanic cell: Pt(s) | H2(1 atm)|H*(1 M) || CI'(1 M) | Hg2Cl2(s)|Hg(l) Which of the…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for…

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Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…

Q: The cell notation for the Galvanic cell is Cd(s)Ca2*/12(s)/" The Standard Reduction Potential are as…

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Q: For the following reaction that occurs at 25°C. 3Zn(s) + 2Cr"(aq) 3Zn2*(aq) + 2Cr(s) (a) Write the…

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Q: 4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the…

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Q: The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×10-3 M and [H*]= 1.11…

A: The formula of calculation of Gibbs free energy is: ∆G=-nFE (a) The chemical reaction taking place…

Q: O ELECTROCHEMISTRY = Understanding concentration cells 13/5 A certain metal M forms a soluble…

A: This question is solved by using the simple concept of electrochemistry which involves oxidation at…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with[Ag+]  = 1.0…

A: The given parameters are: [Ag+]  = 1.0 M molarity of NH3 = 5.0 M  [Cu(NH3)42+] = 0.020 M…