A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.25 V, and ΔGrxn∘ = −44 kJ/mol. If the concentration of Ni2+  is increased to 2.0 M, then Ecell will ______ and Δ????ΔGrxn will be _________ than ΔGrxn∘. Ni(s) + 2H+(aq) ⟶⟶ Ni2+  + H2(g) A) decrease, less negative B) decrease, more negative C) increase, less negative D) increase, more negative

Q: A voltaic cell utilizes the following reaction and operates at298 K:3 Ce4+(aq) + Cr(s)----->3…

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Q: (a) Write the reactions for the discharge and charge of anickel–cadmium (nicad) rechargeable…

A: a.

Q: A certain metal M forms a soluble sulfate salt M₂(SO4). Suppose the left half cell of a galvanic…

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Q: Calculate E, and AG for the following cell reactions at 25 °C. [Mg 2+]= 0.032 M, [Sn 2+]=0.018 M…

A: Answer :- E = 2.22 V , ∆G = -429 kJmol…

Q: An inventor proposes using a SHE (standard hydrogen electrode) in a new battery for smartphones that…

A: A battery is a device composed of two or more two electrochemical cells that convert chemical energy…

Q: 3(a) Balance the following oxidation-reduction equation. NH3(g) + O2(g) → NO(g) + H2O(l) If Br2 is…

A: a) The given reaction is, NH3(g) + O2(g) ---> NO(g) + H2O(l)

Q: Consider the galvanic cell based on the following half-reactions: Zn?+ + 2e -→ Zn e = -0.76 V Fe2+ +…

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Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A: In order for a reaction to run spontaneously, E° cell must be positive, and for the same nickel must…

Q: a. How many grams of NaCl is required to generate a 0.50 L 3.00M NaCl (aq) solution? b. Calculate…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A:

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co…

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Q: The free energy change for the following reaction at 25 °C, when [Cu²+] = 3.44×10-3 M and [Cu²*] =…

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Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+.  Initial concentrations:  [Ni2+] =…

Q: A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in…

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Q: The free energy change for the following reaction at 25 °C, when (Sn2+] = 1.17 M and [Fe2+]…

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Q: What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell…

A: Note: None of the above given reaction is giving correct answer, but by assuming these two reaction…

Q: Heart pacemakers are often powered by lithium–silverchromate “button” batteries. The overall cell…

A: a). The overall reaction for the given battery is, In the above reaction, Li is oxidized to Li+ and…

Q: Patty needs to measure the unknown concentration of Sn2+. A Galvanic cell is set up in a room with a…

A:

Q: Consider a galvanic cell built on the following half-reactions with their standard reduction…

A: The reactions are – Oxidation half cell-2Cr3+ + 7H2O ↔Cr2O7 +14H++ 6e-.....E∘red.=1.33 VReduction…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: When same electrodes of same material used with different concentration then the Galvanic cell is…

Q: Switch KNO, Salt Bridge Cu Sn 1.0 M Cu(NO,), 1.0 M Sn(NO,)2 A student is given a standard galvanic…

A: Oxidation is occuring at the Sn electrode.   Because due to the oxidatio nof Sn to Sn2+ , mass of Sn…

Q: The free energy change for the following reaction at 25 °C, when [Ag"]= 1.19 M and [Ni“]= 2.81×10³…

A: Since the relationship between the free energy change and cell potential is given by  ΔG = -nFEcell…

Q: For cell schematic notation    Zn(s) | ZnCl2 (1.0 M )| | CuSO4 ( 2.0 M ) | Cu(s)…

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Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 1.13 M and [Cr³+] =…

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Q: A galvanic cell based on the reaction below has a measured voltage of 1.37 V. Zn(s) + 2Ag+ → Zn2+ +…

A: Nernest equation gives the relation between cell voltage and concentration of reactants and…

Q: The overall reaction in the lead storage battery is Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4-(aq) →…

A: In this attempt, only the first question is solved according to our answering policy. As, the…

Q: A voltaic cell utilizes the following reaction and operates at 298 K: 3Ce+ (aq) + Cr(s)- → 3Ce+ (ag)…

A: Given reaction is :  3Ce4+ (aq) + Cr (s) ------------> 3Ce3+ (aq) + Cr3+ (aq)  a). What is the…

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e + Mn e° = -1.18 V Fe?+ +…

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Q: Consider a voltaic cell where the anode half-reaction isZn(s)---->Zn2+(aq) + 2 e- and the cathode…

A: Given that: The anode half-reaction is :Zn(s)  →  Zn2+(aq)  +  2e-    E°reduction=-0.76    ....eq 1…

Q: A voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2…

A: Given: Concentration of Fe2+=1.3M Concentration of Fe3+=0.010M pH=3.50 To find: Emf of the cell

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A:

Q: The free energy change for the following reaction at 25 °C, when [Fe²+] = 1.18 M and [Cr³+] =…

A: an electrochemical cell reaction is an example of redox process

Q: A voltaic cell uses the following reaction. Under standard conditions the potential is 2.35 V. What…

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Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag 8° = +0.80 V Cd2+ + 2…

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Q: Consider the following voltaic cell reaction at 25 °C. 2Ag (aq) + Ni(s) Ni2*(aq) + 2Ag(s) -…

A: The Nernst equation is an equation that gives the relation between the standard reduction potential,…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A:

Q: Cu | Cu2+ (0.10 M) || Fe3+ (0.10 M), Fe2+ (0.10 M) | C

A: Given that : Cu|Cu2+(0.10 M) || Fe3+(0.10 M),Fe2+(0.10 M)|C Oxidation is the loss of electrons and…

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A:

Q: What is the cell potential for the reaction at 25oC, if Cl2(g) = 0.100 atm, [Cl-] = 0.100 M, [MnO4-]…

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

Q: MISSED THIS? Read Section 20.6 (Pages 917-922) A voltaic cell consists of a Zn/Zn²+ (E° = -0.76 V)…

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Q: AG° = - â F E° ćel! n FE Consider the following reaction: 3 Pb2+ + 2 Cr(s) → 3 Pb(s) + 2 Cr3+ Using…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to…

A:

Q: How many grams of NaCl is required to generate a 0.50 L 3.00M NaCl (aq) solution?

A: Since you have posted multiple questions, we will solve only first question for you. If you want…

Q: Which metals would act as sacrificial anodes (cathodic protection) for iron? Cr Sn Al Na Cu Despite…

A: lists thes metals as more "active". "more reactive" than…

Q: Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+…

A: Given-> [Fe2+] = 0.00813 M [H2O2] = 0.914 M [Fe3+] = 0.199 M [H+] = 1.32 × 10-3 M

Q: For the Zn-Cu2+ voltaic cell, we have Zn (s) + Cu2+ (aq, 1 M) → Zn2+(aq, 1 M) + Cu (s) Ecell 0 =…

A: To find electrode potential.

Q: MnO4– + Sn ---> MnO2 + Sn2+ a) What is the half reaction that takes place at the cathode? b) What…

A: Recall the given reaction       Mn7+O4- + Sn0 → Mn4+O2 + Sn2+ Recall values of standard electrode…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 2.57x10-³ M and [I₂] =…

A:

Q: Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the…

A: Ecell is calculated using nernest equation.  For this first we would calculate E°cell using standard…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.