Order the following oxidizing agents by increasing strength under standard-state conditions:  1. Ag+(aq) 2. Cd2+(aq) 3. MnO42-(aq) in acidic conditions The standard reduction half-reactions and standard reduction potentials for the above species are as follows: 1. Ag+(aq) + 1e- <=> Ag(s)     Eo = +0.80 V 2. Cd2+(aq) + 2e- <=> Cd(s)   Eo = - 0.40 V 3. MnO4-(aq) + 8 H+(aq) + 5e- <=> Mn2+(aq) + 4 H2O(l)    Eo = + 1.49 V

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: EFM of the cell is calculated by using below formula,

Q: Consider the electrolysis reactions cathode Cu?"(aq, 0.177 M) + 2e-= Cu(s) H,O) =0,(g, 1 bar) + 2H*…

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Q: A chemical reaction system is represented by this equation. Ag(s) + Br(aq) + Fe3+(aq) → Fe2+(aq) +…

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Q: The standard reduction potentials for zinc and silver are     Ag (aq) + e -> Ag (s)   Eo = +0.80 V…

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Q: Calculate the standard free energy change for the following reactions using the standard cell…

A: We need to divide the given reactions into two half-cell reactions and use the Standard reduction…

Q: Calculate AG° for the following cell reaction: TI(s) | TI* (aq) || Ni²* (aq) | Ni(s) From AG°,…

A: For a galvanic cell, the relation between Gibbs free energy and potential is  :ΔG°cell= −nFE°cell…

Q: For the reaction: Pd2+ + Ni → Ni²+ + Pd , AG° is –239 kJ/mole. What is the standard reduction…

A: The tendency possessed by ions to get reduced in any reaction is termed as its "standard reduction…

Q: Use the appropriate standard reduction potentials below to determine the equilibrium constant at 326…

A: Given : 1) Net reaction : 4H+(aq) + MnO2 ​(s) + 2Fe2+(aq) -----&gt; Mn2+(aq) + 2Fe3+(aq) + 2H2O(l)…

Q: 2(g) |H '(aq) || Pb<'(aq) | PBS04(s) | Pb(s) he following standard reduction potentials. q) + 2 e¯ ®…

A: Cell equation,  Sn2+ + Cu2+ ---&gt; Sn4+ + Cu Cell potential is affected by concentration.  As the…

Q: + Zn(s) → 2Hg() + ZnCl2 (aq, 0.0050m) -323 J/mol at all temperatures) E° = -0.76 V Cl(aq) E° = 0.27…

A: From the standard reduction potential data, E°cell = E°c - E°a

Q: The value of K, for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br°(aq)…

A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq)       E°=0.070 V The Ksp value 5.4×10-13

Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

A: Here we are required to find the cell potential of the given two electrochemical reaction

Q: )    Using a table of standard electrode potentials, predict whether the following reactions will be…

A: There is something incorrect in equation of part c so it can't be solved For a spontaneous reaction…

Q: Cr3+ (1 M) Cr2+ (1 M) T13+ (1 M) T13+ (aq) + 3e-> TI (s) Cr2 (aq) Cr3 (aq) + e- Using the list of…

A: Given reaction :  E°cell = +1.14 V Reduction half Reaction takes place at Cathode Tl3+ (aq) + 3 e-…

Q: Given the following standard reduction potentials: Mg+2 = Mg(s) + 2e- E = (-) 2.37 V 2e- + I2(s) =…

A: Dear student the first equuation for Mg given is wrong as Mg2+ ion can never give Mg and 2 e- .

Q: (E°cell

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Q: What is E°(cell) for the cell Mn | Mn²⁺(aq) || Ag⁺(aq) | Ag?   Standard Reduction Potential: Au³⁺(aq…

A: Thank you.

Q: The cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

A: The cell potential is calculated by Nernst equation . E = E° - (0.0591/n) log Qc E = cell potential…

Q: Calculate the standard cell potential, E°cell, for the following reaction, and indicate if the…

A: We are given a redox reaction happening in an electrochemical reaction. The oxidation half-reaction…

Q: Calculate the standard cell potential, Ecell, for the equation Fe(s) + F₂ (g) Fe2(aq) + 2F (aq) Use…

A: As per standard reduction table Fe2+(aq)  + 2e- → Fe(s)              E° = -0.44 F  F2 (g)+ 2e- → 2F-…

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

A: given data are-  Fe(s) ⟶ Fe2+(aq) + 2e-Eo = -0.44 V  O2(g) + 4H+(aq) + 4e- ⟶  2H2O(l)  Eo = 1.23 V…

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: For a spontaneous reaction, the cathode must have higher electrode potential than the anode. The…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: In the galvanic cell , two half Reaction occur . One at anode and one at cathode . When both the…

Q: Calculate the standard state cell potential for the reaction below given the standard reduction…

A: To solve this problem we need to write the oxidation half and reduction half reaction and  According…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: equilibrium reaction is  Sn+2(aq) + 2 Fe+3(aq)   &lt;--&gt;  Sn+4(aq)   + 2 Fe+2(aq)  (1)…

Q: X(s)|X5+ (0.94 M) || Mn O4 1 minus (1.10 M)|Mn O2(s)|H+ (0.51 M) The reduction potential for X5+ is…

A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

Q: The voltaic cell described by the notation below measured a potential of 1.1 V. If the reaction was…

A: The given cell notation for the voltaic cell is:- Pt(s) | J2- (1.50 M) | J(l) || Ag+ (0.010 M) |…

Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.36 V; Zn2+ (aq)|…

A: The standard half cell reactions are    Cu+2 (aq)+ 2 e− ⇌ Cu (s)    E° = 0.29 V    Cd+2 (aq)+ 2 e− ⇌…

Q: Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard…

A: Given: Half-cell reactions: Cu+2 (aq) + e- → Cu+ (aq)     Eo = +0.15 V V+2 (aq) + 2e- → V (s)…

Q: Consider the following electrochemical cell in which X is an unknown metal:        Pt (s) | Cl–(1 M)…

A: Given :-  The given electrochemical cell  Standard cell emf = E0 = 0.23 V  Temperature = 25 oC…

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: sing the following standard reduction potentials: Ag+ (aq) + e- ⇌ Ag (s) E o = +0.80 V Pb2+ (aq) +…

A: Electrons flow from anode to cathode anode is negatively charged and cathode is positively charged .…

Q: Given: Br2 (1) + 2e 2 Br-1 12 (s) +2e=21-¹ O-1.63 V What is the standard cell potential for the…

A: The standard cell potential of any reaction is defined as the difference between the potential of…

Q: Calculate Ecell for the following cell: Pt(s) | H2(g) | H *(aq) || Pb2*(aq) | PBSO4(s) | Pb(s) given…

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Q: Calculate E° cll from the tabulated standard reduction potentials for each of the following…

A: In the given reaction MnO4- is getting reduced while Fe+2 is getting oxidised.

Q: Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1…

A: Here, in the given cell notation, first of all the notation has to be understood. Pt | Cl- (1 M) |…

Q: If the concentration of Ag* is 0.0115 M, the concentration of H* is 0.355 M, and the pressure of H2…

A: Use Nernst equation, to get the cell potential:

Q: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: The Nernst  equation is given as :

Q: A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M…

A: