Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E o      (Fe2+ / Fe) = −0.4400 V, E o      (Cd2+ / Cd) = −0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.75 M and [Cd2+] = 0.010 M. E =     V Will the reaction occur spontaneously at these conditions?    yes    no    cannot predict

Q: Why is it necessary to use the standard hydrogen half-cell as a reference when calculating standard…

A: Given statement is :  Why is it necessary to use the standard hydrogen half-cell as a reference when…

Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

A: Given: The overall cell reaction will be as follows: 2H+(aq) + Zn(s)---------> H2(g) + Zn2+(aq).…

Q: Calculate the standard emf for the following reaction at 298 K. Cd(s) + 2 Co3+(aq) - Cd2+(aq) + 2…

A: From the value of standard reduction potential we can identify which species will oxidise and which…

Q: Define Galvanic Series.

A: Galvanic series has to be defined. The galvanic series is predominant for selection of material to…

Q: Consider the following reaction at 298K. 2Fe³+ (aq) + Fe(s) 2Fe2+ (aq) + Fe²+ (aq) The standard…

A:

Q: Calculate the standard free-energy change at 298K for the zinc-copper voltaic cell, which has a…

A:

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: 2 Cr(s) + 3 Cu*2(aq) → 2 Cr*³{aq) + 3 Cu (s) E° = 0.43 V Which expression gives the value for AG" in…

A:

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: How is equilibrium constant of a reaction related to standard cell potential?

A: How is equilibrium constant of a reaction related to standard cell potential?

Q: Comment on the sign of Δ S system for the following reaction.Fe(s) + Z n 2+ (aq) → F e 2+ (aq) +…

A: Entropy of a chemical reaction is predicted by the randomness taking place in the system. Entropy of…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Co(s)→→→ Hg(t) + Co²+ (aq) The standard Gibbs…

A: Given-> ∆G° = -219.06 KJ = -219.06 × 1000 J = -219060 J

Q: Consider the cell Pt(s)/ H2(g, 1 bar)/NaOH (aq, 0.01m), NaCl (aq, 0.01125m)/ AgCl(s) / Ag(s) 2H₂O +…

A: Recall the cell representation,                           Pt s / H2 g, 1 bar / NaOH aq, 0.01 m,…

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

A:

Q: A. Calculate the standard free-energy change at 25 ∘C for the following reaction:…

A:

Q: The cell potential for a given reaction is -0.04 V. Calculate the Gibbs energy and equilibrium…

A: 1.) Gibbs free energy can be calculated using given cell potential using formula : ∆G = - nFEocell…

Q: Determine the equilibrium constant at the following reaction at 298 K. 2 Fe3+ + Sn2+ 2 Fe2+ + Sn4+…

A:

Q: 0.0592 V E cell -log(K) Calculate the equilibrium constant for the following reaction at 25°C:…

A: E°cell = (0.0592 V / n ) × log(K) 2Ag(s) + Fe2+(aq) <---> 2Ag+(aq) + Fe(s)  K = ?

Q: 4. Calculate the Gibbs Free-Energy and the standard Gibbs Free- Energy by the cell in the given cell…

A: Given : [Zn+2]  = 4.0 x 10-3 M  [H2] = 0.010 M  [H+] = 1.0 M  Also,  E°Zn+2/Zn = - 0.76 V  E°H+/H2 =…

Q: Fe2* (aq) + Cr** (aq) 2 Cr²* (aq) + Fe** (aq) Cr** (aq, 1.0 M) +e¯ → Cr²* (aq, 1.0 M) E° =-0.41 v…

A: When direction of reaction is reversed then the concerning sign of the electrode potential also gets…

Q: You are investigating a catabolic pathway in the cell. Refer to the different reactions be Reaction…

A:

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

A:

Q: Consider the following galvanic cell: Ag(s) | Ag*(3.0 × 104 M) || Fe³*(1.1 × 10³ M), Fe²*(0.040 M) |…

A: Given,

Q: Consider the following reaction at 298K. Ag" (aq) + Cu (aq) Ag (s) + Cu²+ (aq) - Which of the…

A: The half cell reactions are: Anode: Cu+(aq) →Cu2+(aq) + e-                            E° = 0.16…

Q: Calculate DG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C)…

A:

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

A: It is an example of electrochemical reaction  Here we are required to find which of 3 quantities are…

Q: Consider the following reaction at 298K. 2+ Hg (aq) + H2(g) Hg(f) + 2H*(aq) The standard Gibbs free…

A: Hg2+ (aq)  +  H2(g)   →  Hg(l)  + 2H+ (aq)Oxidation half cellH2(g)   →2 H+(aq)+ 2 e-Reduction half…

Q: By what ratio will Q change if the cell potential is increased by 0.63 V? Assume v = 1 and the…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

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

A: (a)

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

A:

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: Consider the following cell diagram: Cool Co2+ (aq) (0.015 M) | Fe2+ (1.94 M)| Fes) (aq) What is the…

A: The cell potential will given by Nernst Equation:

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

A:

Q: A nonstandard cell is made by replacing the 1.0 M solutions of Cu(NO3)2 and Sn(NO3)2 in the standard…

A: Answer: 1. Let the standard electrode potential 1 M solution of Cu(NO3)2 and Sn(NO3)2 be E0 So,…

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

A:

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

A:

Q: 3. Assuming standard states for all reactants and products, determine the spontaneous direction of…

A: The reactions given are, 1) Cu + 2 HCl → CuCl2 + H2  2) Ag + FeCl3 → FeCl2 + AgCl

Q: Give the equilibrium constant for the following reaction at 298 K.

A: In the given cell reaction, cupric ion is being reduced to copper and Sn+2 is being oxidized to…

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: Using the information in the data section, calculate the standard reaction ent and standard reaction…

A: Given reaction is :  N2 (g) + 3H2 (g) ---------> 2NH3 (g)  a). Calculate the standard change in…

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: Cd(s) + Fe2+(aq)  →  Cd2+(aq) + Fe(s) E o      (Fe2+ / Fe) = −0.4400 V, E o…

A: The Nernst equation relates the cell EMF to standard cell potential. At 298 K, the nernst equation…

Q: f the potential of a galvanic cell is +1.20 V, what is the Gibbs free-energy change when one mole of…

A: Given  potential of a galvanic cell is +1.20 V when one mole of electrons is transferred in the…

Q: Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard…

A:

Q: The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction…

A: In case of lactic acid the no. of moles of acid is equal to the no. of moles of hydroxide ion that…

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

A: Given :