Observe this cell at room temperature: Co(s) + Fe2+(aq.) (1.94M) ⟶ Co2+(aq.) (0.15M) + Fe (s) Is the process spontaneous? E∘Co2+/Co=−0.28 V, E∘Fe2+/Fe=−0.447 V

Q: A student made measurements on some electrochemical cells and calculated three quantities: • The…

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Q: ustify the following statement 1. EMF of a cell is always positive. 2. Zinc displaces copper from…

A: 1. EMF of a cell is always positive - False, it can be negative also. 2. Zinc displaces copper…

Q: For the electrochemical cell: M| M* || X- | X, E° [M* | M] = +0.44 V and E° [X | X] = +0.33 V. A M*…

A: To check the spontaneity of electrochemical reaction, we have to determine the value of E°cell.…

Q: Consider the reaction in the lead-acid cell      PB(s) + PbO2(s) + 2H2SO4(aq)  2PbSO4(aq) + 2H2O(l)…

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Q: Calculate: (a) the pH of the saturated solution of magnesium  hydroxide:   Mg(OH)2(s) →← Mg2+(aq) +…

A: Mg(OH)2 ⇌ Mg2+ + 2 OH¯ Ksp = [Mg2+] [OH¯]2 Ksp =1.2 x 10¯11 = (s) (2s)2 ksp = 4s3 After dividing by…

Q: The value of the equilibrium constant for the reaction of nickel(11) ions with cadmium metal is 1.17…

A: Suppose an Equilibrium reaction A2(g) +B2(g) ⇌2AB(g)Equilibrium constant (k) = Product…

Q: The free energy available from a 1.10-volt Cu(II)-Zn cell under standard conditions is   -212 kJ…

A: Given that: Standard electrode potential of cell = 1.10 V To find: Standard Gibbs free energy =?

Q: From the thermodynamic data, ΔSsys for the given fuel cell reaction is negative but the reaction is…

A: The reason the negative entropy of the system can be justified as spontaneous has to be explained.…

Q: Under standard conditions, the electromotive force of the cell, Zn(s) | ZnCl₂(aq) | Cl₂(g) | Pt is…

A: Solutions  Hence the standard entropy of the formation - 1.384 kj/mol

Q: If E° for X + e– → Y is larger than E° for A + 2e– → B, then in a spontaneous process under…

A: The substance which has tendency to oxidize others and reduce itself is known as oxidizing agent.…

Q: Consider the following reaction at 298K. 2 H* (aq) + Zn (s) H2 (g) + Zn²* (aq) Which of the…

A: The given reaction is, 2H+ (aq) + Zn (s) ----->H2(g) + Zn2+ (aq) Two half reactions for the given…

Q: how much does the cell potential change when Q is decreased by a factor of 10 for a reaction in…

A: Given , valence factro(v) = 2 T = 298 K Q is decreased by 10 Using Nernst's equation,  E1 = E° -…

Q: A certain metal M forms a soluble nitrate salt M M(NO3)₂. Suppose the left half cell of a galvanic…

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Q: Solve the given problems with complete solution. Calculate the Gibbs Free-Energy and the standard…

A: we are required to find the Gibbs free energy and standard Gibbs free energy for the given cell…

Q: (a) The discharge reaction for a zinc-manganese dioxide battery can be represented as: Zn(s) +…

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Q: 1. Calculate the emf generated, Gibbs Free-Energy and the standard Gibbs Free-Energy by the cell in…

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Q: A student made measurements on some electrochemical cells and calculated three quantities: • The…

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Q: standard conditions Express your answer in units of volts. Ecell= 2.33 V Calculate the cell…

A:

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

A: (a)

Q: 5. For the cell Cd(Hg)|CdSO4 H2O(s)|Hg;SO4(s)|Hg the emf is given as a function of temperature t…

A: The emf as a function of temperature is given as, => E (V) = 1.01845 - 4.05 X 10-5 X (t - 20) -…

Q: Given the included data, calculate AG° and K at 298 K for the oxidation of nitrite 1on to nitrate…

A: Change in standard Gibbs free energy and equilibrium constant calculation:

Q: Consider the reaction given below at 25 degrees Celsius and answer the questions that follow. (A).…

A: An electrochemical cell undergo both oxidation and reduction process at the same time at respective…

Q: The standard voltage, Eº, for the reaction of Zn(s) and Cl₂(g) is 2.12 V. What is the standard Gibbs…

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Q: = +0.851Vwhat is the spontaneous reaction between these two half-cells and what is the poten

A: For Spontaneous reaction, E°cell is positive.  Electrode with higher standard reduction potential…

Q: Gibbs energy change, A:G®, is related to cell potential, E, by the equation Calculate the standard…

A: For the given cell, change in enthalpy and entropy at 25oC is as follows: ∆rHo = -729 kJ mol-1∆rSo =…

Q: By how much does the cell potential change (in volts) when Q is increased by a factor of 21 for a…

A: Answer:

Q: 6.1 Is the transport of Na* ions across a cell membrane spontaneous when [Na"]in/[Na*]out = 0.10 and…

A: [Na]in /[Na]out=0.10 An ionic imbalance is present here.

Q: The standard voltage, E°, for the reaction of Zn(s) and Cl,(g) is 2.12 V. What is the standard Gibbs…

A: Standard gibb's free energy is directly related to Standard EMF of the cell.  Here ,Zn2++2e-→Zn and…

Q: Q.4. Calculate the standard Gibbs free energy change, AG°, at 250C for the following reaction.…

A:

Q: The cell whose diagram is Pb(s) I PbCl,(s) I KCI(aq) I Hg,Cl,(s) I Hg(1) Has a standard emf of…

A: Given :  E°cell = 0.5359 V  Temperature coefficient = 1.45 x 10-4 V/K  T = 298.15 K

Q: consider the following tin-permanganate cell: Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq)…

A: The cell given is Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq) (0.022 M) | MnO2 (s).

Q: The redox potentials for the Zn2+/Zn and Cl2/Cl– couples are -0.764 V and 1.395 V, respectively.…

A:

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18 h. If 4.33…

A:

Q: 21. Use the data given below to calculate AG (in kJ/mol) for the following cell reaction at 25 °C:…

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Q: Using the electrochemical data found at the top of the Canvas page, calculate the equilibrium…

A: Given reaction is :  In (s) + Md3+ (aq) <----------> In+ (aq) + Md2+ (aq)  Calculate the value…

Q: Calculate Eºcell (in V) and indicate whether the reaction shown is spontaneous or nonspontaneous…

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Q: Cassandra builds a galvanic cell using a zinc electrode immersed in an aqueous Zn(NO3)2 solution and…

A: Given,  zinc electrode immersed in an aqueous Zn(NO3)2 solution and an copper electrode immersed in…

Q: Saquon builds a galvanic cell using a zinc electrode immersed in an aqueous Zn(NO3)2 solution and a…

A: The anode , oxidation takes place. So to check which species is produced at anode , we first check…

Q: What is the standard Gibbs free energy change and equilibrium constant when Ag+ reacts with iron to…

A: Given: Ag+ reacts with iron to form iron(II) at 25oC. To answer: Writing a balanced chemical…

Q: 6. For the cell Cd(Hg)|CdSO,. H,0(s)|Hg,SO,(s)|Hg the emf is given as a function of temperature t…

A: Given : E(V) = 1.01845 - (4.05x10-5)(t-20) -(9.5x10-7)(t-20)2  We have to calculate : ∆G , ∆H , ∆S

Q: Write the schematic representation and reaction of the cell composed of SHE and cadmium electrodes.…

A: The electrode which has higher reduction potential acts as a cathode and the electrode with lower…

Q: Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)…

A: The relationship between the ΔGrxn and Q is: Given data: ΔG° =-28.0KJ. P(CO) =4.2atm, P(CO2)=1.8atm…

Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

A: Interpretation - To write the half cell reaction that occurs at each electrode To check here which…

Q: (a) What is the value of E° for the following reaction? Zn2*(aq) + Ni(s) → Zn(s) + Ni2*(aq) (b) Is…

A: We can determine the standard cell potential of any cell from the following formula : E 0 cell  = E…

Q: å. Calculate A for the following reaction át 298 K. ClO; (aq) + 5 Cl¯ (aq) + 6 H† (aq) → 3 Cl2 (g) +…

A: Given :

Q: Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →…

A: Given cell reactions with E0 values: Sn4+  +  2 e−   →   Sn2+    E0 = 0.139 V Ag+  +  e−   →   Ag(s)…

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.