Oxidation-reduction potential of the system MnO4 +8H*/Mn**+ 4H,O decreases, in case of: MnCl, addition KCl addition Temperature increasing KMNO4 addition
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2+(aq) +…
A: Standard electrode potential value of the given cells are as follows E°Cu2+/Cu =0.337 V and…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+(aq) +…
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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: The following reduction potentials are measured at pH 0: BrO, + 6 H,O* + 5 e →B12 (e) + 9 H20 E° =…
A: The E0cell of the reaction is calculated as follows:
Q: Calculate the cell potential at 25°C for the cell Fe(s) ∣ (Fe2+(0.100 M) ∣∣ Pd2+(1.0 ×…
A: The cell given is Fe(s) ∣ (Fe2+ (0.100 M) ∣∣ Pd2+ (1.0 X 10-5 M) ∣ Pd(s) Since the oxidation half is…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2+(aq)…
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Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H*(aq) +…
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Q: he reduction potentials for Au 3+ and Ni 2+ are as follows: Au3+ + 3e– → Au, ε° = +1.50 V Ni2+ + 2e–…
A: The reduction potential half cells for Au3+ andNi2+ are given belowAu3++3e-→Au…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2+(aq) +…
A: Given reaction: This reaction occur in room temperature as in question…
Q: Below are values for the standard reduction potentials for various species of the metal, M: MO₂2²+ +…
A: Frost diagram represent the graphical method of summarising redox relationship for species…
Q: e) Determine the Gibbs energy change per mole of reaction. Faraday's constant is 96485 reduction…
A: Anodic reaction: C2O42- -----------> 2CO2 + 2e- ---------(1)…
Q: For the galvanic cell at 298 K 2Cr(s) + 3NI2+(aq) 20r3+(aq) + 3Ni(s) cell = 0.51 V What is the…
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Q: Given the following standard reduction potentials, Pb2+(aq) + 2 e → Pb(s) E° = -0.126 V PBSO4(s) + 2…
A: First the standard cell potential value is calculated from given reduction potentials.
Q: Balance the following reaction under acidic conditions and calculate cell potential at 298K Cr2072…
A: BALANCING OF REDOX REACTION Cr2O7-2 + 6I-1 + 14H+→2Cr+3 + 3I2 + 7 H2o
Q: The cell potential of the reaction: PbSO4(aq) + Cr(s) ⇒ Pb(s) + Cr²+ (aq) + SO4²- (aq) is +0.55 V.…
A: Reducing agent is the substance which reduces others and oxidize itself. Oxidizing agent is the…
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: At 25 ∘C,25 ∘C, a titration of 15.00 mL of a 0.0320 M AgNO3 solution with a 0.0160 M NaI solution is…
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Q: The following reduction potentials are measured at pH 14: CIO" + H¿O + 2 e¯ → Cl¯ + 2 OH¯ E° = 0.90…
A: Given reaction
Q: Calculate the cell potential, ∆G, and equilibrium constant for the reaction Ca(s) + Mn2+(aq) (1M) ⇌…
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Q: calculate the potential of platinum elctrode emersed in a solution 0.0613 M in k4Fe(CN)6 and…
A: The concentration of k4Fe(CN)6=0.0613 M The concentration of k3Fe(CN)6=0.00669 M The oxidation…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2+(aq) +…
A: First we have to find EoCell for the reaction, and then from EoCell we can find equilibrium…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2*(aq) +…
A: In this question determine E°cell. ∆G° = -nFE°cell also ∆G° = -2.303 RT log K
Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…
A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…
Q: Given the following standard reduction potentials: MnO4 (aq) + 8H*(aq) + 5 e - - Mn2*(aq) + 4 H20()…
A: The expression of Nernst equation is shown below: E =E0cell -0.0591n log Q Where; Ecell= cell…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2 *(aq)…
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Q: Under standard conditions (250 C, 1.0 atm): i. If Cr metal is immersed in a solution of Zn(NO3)2,…
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Q: Pt(s) Br (aq) (x M) | Br21) || BrO3¯(aq) (0.43 M), H*(aq) (1.00 M) | Br2(1) | Pt(s)
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Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + With(so much) =…
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Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Ni²*(aq) +…
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Q: Given that standard reduction potentials at 298.15 K are E° Ag+ /Ag = +0.800 V and E° Cu?"/Cu =…
A: When Ag foil is soaked into Cu(NO3)2 solution, for Ag to dissolve the reaction involved would be:…
Q: A cell is constructed by coupling a Zinc electrode dipped in0.5M ZnSO4 and a Nickel electrode dipped…
A: Given concentration of Zn2+ is 0.5M. concentration of Ni+2 is 0.05M Standard reduction…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg*(aq) +…
A: In a redox reaction, one species undergoes oxidation while the other species undergoes reduction.…
Q: Fe(s) I (Fe2+(0.100 M) || Pd2+(1.0 x 10-5 M) I Pd(s) given that the standard reduction potential for…
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Q: Jse standard reduction potentials to calculate the equilibrium constant for the reaction: Ca²*(aq) +…
A: The half reactions taking place are Oxidation : Cu (s) ---------> Cu2+ (aq) + 2 e-…
Q: The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal (M)…
A: Given: Cell potential (Ecell) = -0.265V PH2 = 0.40 bar pka values of citric acid = 3.128, 4.761 and…
Q: Calculate the reduction potential for a Pt | Cr3+, Cr2+ halfcell in which [Cr3+] is 0.15 M and…
A: In inorganic chemistry, reduction is the process of gaining of electrons during the reaction.…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2+(aq) +…
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Q: Standard Reduction Potentials Sn*(aq) + 2e → Sn²*(s) E° = 0.15 V K"(aq) + le → K(s) E° = -2.92 V |3D…
A: Given: One ampere current is passed through an aqueous solution of Ni(NO3)2
Q: The standard free energies of formation of several species are: kJ/mol H+(aq) 0 H2O(l) –237.0…
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Q: By considering these half-reactions and their standard reduction potentials, Pr2+ + 2 e -→ Pt E° =…
A: In a redox reaction a half cell reaction is either reduction or oxidation component of reaction. For…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2+(aq) +…
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Q: Given that standard reduction potentials at 298.15 K are E° Mg*2 /Mg = -2.37 V and E° Sn2*/Sn =…
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Q: Calculate the electrode potential of a silver electrode immersed in a 0.2500M solution of KCl using…
A: Given - E0 Ag+/Ag=0.799v E0 AgCl/Ag=0.222v KCl = 0.2500 M To find - electrode potential of a silver…
Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Sn2+(aq) +…
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Q: Calculate the electrode potential of a silver electrode immersed in a 0.2500M solution of KCl using…
A: Given - E0 Ag+/Ag=0.799v E0 AgCl/Ag=0.222v KCl = 0.2500 M To find - electrode potential of a silver…
Q: Acidic solution s,0,2- + MnO, → SO,?- + Mn²+ compensate for the redox reaction
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Q: The standard reduction potential (Eo) for the conversion of Cr2O72- to Cr3+ at 25 degree C in an…
A: A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction…
Q: Given the hypothetical metal samples a, B. and y were placed in an electrochemical cell as…
A: E°alpha = ? E°gamma = -2.38 V
Q: Calculate Gibbs free energy change (G) for the following reaction Zn+Cu+2 Zn+2 +Cu when [zn2+]= 10…
A: The Gibb's free energy of a cell depend on the reduction potential of a cell. It will describes the…
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- The standard free energies of formation of several species are:kJ/molH+(aq) 0H2O(l) –237.0CH3OH(aq) –163.0HCOOH(aq) –351.4e– 0What is the standard reduction potential (Eo)of methanoic acid in aqueous solution (i.e., for HCOOH + 4H+ + 4e– →CH3OH + H2O)?Calculate Gibbs free energy change (G) for the following reaction Zn+Cu+2 Zn+2 +Cuwhen [zn2+]= 10 M and [cu2+]= 1M at 25oC, F = 96.5 KJ/ Vol.molif you know that reduction potentials are as follow: Zn2+ +2e-Zn Eo=-0.76VCu2+ + 2e-Cu Eo= 0.34 VUse standard reduction potentials to calculate the equilibrium constant for the reaction:2Ag+(aq) + H2(g)2Ag(s) + 2H+(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant: G° for this reaction would be than zero
- Consider the reaction shown here occurring at 25∘C Cr(s)+Cd2+(aq)→Cr2+(aq)+Cd(s) Determine the value of Ecell∘, K, ΔGrxno for the reaction and complete the table.E∘ for the reduction of Cr(II) is −0. 91V [Cd2+](M) [Cr2+](M) Q Ecell ΔGrxn 1.00 1.00 1.00 1.00×10−3 1.00×10−3 1.00 5.66× 10−4 1.00At 25 ∘C,25 ∘C, a titration of 15.00 mL of a 0.0320 M AgNO3 solution with a 0.0160 M NaI solution is conducted within the cell SCE || titration solution | Ag(s)SCE || titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of NaINaI solution? The reduction potential for the saturated calomel electrode is ?=0.241 V. The standard reduction potential for the reaction Ag++e−⟶Ag(s) is ?∘=0.79993 V The solubility constant of AgI is ?sp=8.3×10^−17. 0.200 mL?= 19.00 mL?= 30.00 mL?= 43.20 mL?= please solve3. Determine the oxidationnumber for the indicated elementin each of the followingsubstances: (a) S in SO2 , (b) Cin COCl2 , (c) Mn in MnO4- ,(d)N in N2H4 , (e) N in HNO2 ,(f) Cr in Cr2O72-
- calculate the potential of platinum elctrode emersed in a solution 0.0613 M in k4Fe(CN)6 and 0.00669M in k3Fe(CN)6Consider the half reactions shown below with their associated standard reduction potentials at 25 ∘C PbI2(s)+2e− → Pb(s)+2 I−(aq) Ered∘ = –0.34 V Pb2+(aq)+2e− → Pb(s) Ered∘ = –0.13 V A.) Use the given information to calculate KspKsp for the dissolution of PbI2(s) at 25 ∘C B.) Calculate ΔG∘ for the dissolution of PbI2(s) at 25 ∘CFor the reaction, 2CuI(s) + Cd(s)--->Cd2+ + 2I-(aq) + 2Cu(s), E0=0.23V. Given that E0Cd2+/Cd=-0.403V, determine E0 for the half reaction.
- The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell. Result: a) Eºcell >0 d) 0.7108 V, 0.7482 VThe reduction potentials for Au3+ and Ni2+ are as follows: Au3+ + 3e Au, E = +1.50 V Ni2+ + 2e Ni, E = -0.227 V Calculate AG (at 25°C) for the reaction: 2AU3+ + 2Ni +3Ni2+. + 2AuCalculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X1 (where X is the anion) with a supplied current of 4.1 A for 9 h, consuming 0.2027 kWh of electrical energy. Assume that the current efficiency is 93%.
