Calculate Ksp for zinc sulfide from the following data: ZnS(s) + 2e - Zn(s) + S?- (aq) e = -1.41 V 2+(ag)+2e → Zn(s) Zn e° = -0.76 V Ksp =

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

Q: Consider an electrochemical Given that the Ksp of FeCO3 is 3.5 x 10-11, what would be the expected…

A: Interpretation - In the given question here we have to determine the Ecell  of the given…

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: An iron(II) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with…

A:

Q: Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate…

A:

Q: Cadmium sulfide (CdS) is used in some semiconductor applications. Calculate the value of the…

A: Recall the given redox reactions,CdS  +  2 e-  →  Cd  +  S2-                            ؏° = -…

Q: 19. Given Fe + 2e → Fe, o° =-0.440 v, and Fe +eFe", o° = 0.771 V, cal- culate o° for Fe* + 30 Fe 20.…

A: 19)  Fe2++2e - ➡️ Fe.        ¢°=-0.440V       Fe3+ +e- ➡️Fe2+.         ¢° =0.771V Adding both the…

Q: The standard reduction potential for Zn2+ is -0.76 V. Calculate the voltage of the following cell at…

A: The reaction at anode i.e oxidation, Zn(s)------------>Zn2+(aq)+2e-........................E0=…

Q: A cell was prepared by creating the following cells: Anode: a Zr wire in a 1 M Zr4+ solution (Zr4+…

A:

Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…

A:

Q: What are the products at the cathode and anode when an aqueous solution of KI is electrolyzed…

A:

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag*(aq) +…

A:

Q: Calculate the equilibrium constant, ,K, for the reaction shown at .25 °C.…

A: Given: The equation is given below as,

Q: Based on the information in the table of standard reduction potentials below, calculate AG° for the…

A: The half-cell reactions for the given reaction is as follows:

Q: 2. a platinum electrode immersed in a solution that is 0.0400 M in Fe2SO4 and 0.00915 M in Fe2(SO4)3…

A: Here we have to determine electrode potential of the following half electrodes.

Q: Consider the half reactions shown below with their associated standard reduction potentials at 25 ∘C…

A: First of all we have to calculate the cell potential of the overall reaction.

Q: For the galvanic cell at 298K 2Cr(s) + 3NI2*(aq) --> 2Cr3+(ag) + 3Ni(s) E°cell = 0.51 V What is the…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation.  Hence when a…

Q: Calculate the equilibrium constant, ?, for the reaction shown at 25 °C.…

A: Given Fe3+(aq)+3e−⟶Fe(s)   E = −0.04 V H3BO3 (s)+3H3O+(aq)+3e−⟶B(s)+6H2O(l) E = -0.8698 V  T = 298 K

Q: For the galvanic cell at 298 K 2Cr(s) + 3NI2+(aq) 20r3+(aq) + 3Ni(s) cell = 0.51 V What is the…

A:

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 equilibrium constant, Kc, was found to be 1.3 x 10^3 at 24.6 C for the reaction.…

A: Here we are required to find the reduction potential of half reaction of X.

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) +…

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Q: A mixture of copper and gold metals that is subjected toelectrorefining contains tellurium as an…

A: Given information:

Q: A galvanic cell consists of a Cr+/Cr half-cell with unknown [Cr³+] and a Ni²+/Ni half-cell with…

A: GALVANIC CELL: It is a type of an electrochemical cell which is utilized to provide electricity by…

Q: Using the Half-Reaction method, balance the following Redox equation in an acidic aqueous solution:…

A:

Q: Given the electrochemical reaction shown, what is the standard free energy change AG° if E° = +1.61…

A: ∆G° = - n F Eo n= The elctrons transfered from anode to cathode in the cell = 2. F = 96500 columbs.…

Q: At 25 °C, calculate the voltage of the cell 2Ag*(aq, 0.10M) + Cu(s) → Cu²*(aq, 0.010M) + 2Ag(s) If…

A:

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Ca²"(aq) +…

A: In this question, we will determine the Equilibrium constant for this reaction and also determine…

Q: Use the standard reduction potentials given below to predict if a reaction will occur when Pb metal…

A: Here we are required to find whether a reaction is possible when pb metal is added to Mn2+ solution.…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd²*(aq) +…

A: Cd2+ + 2 e-    -------->   Cd                      ( at cathode )          Co…

Q: (4) CuSO4 is electrolyzed for 10 minutes with 5.1 A current, calculate mass (g) of Cu deposited? B)…

A: The Faraday's first law of electrolysis states that, the amount of compound deposited at electrode…

Q: On the diagram below sketch the regions where colour has developed and what colour each region is…

A: Sacrificial anodes protect metals from corrosion, it works by oxidizing more quickly than the metal.…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + With(so much) =…

A:

Q: 5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ),…

A: The molar mass Fe atom is:- 55.85g/mol

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…

A:

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V  PH2=0.857atm Concentration of Cd2+=1.00M

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2*(aq) +…

A: The half reactions taking place are  Reduction : Co2+ (aq) + 2 e- ------> Co (s)…

Q: Consider the following reaction and their reduction potential values: Cu+ + Ni2+ —> Cu2+ + Ni…

A: Overall Cell potential  Spontaneity

Q: An electrolytic cell contains 50.0 mL of a 0.297M solution of Fe Cl3. A current of 0.643 A is passed…

A: First, calculate the Faradays represented by 0.643 A for 15.0min as follows: Faradays = 0.643C s ×…

Q: Calculate the time required for a constant current of 0.885 A to deposit 0.335 g of TI(III) as TI(s)…

A: This question is related to Faraday law.

Q: 3. A galvanic displacement is now happening between Zn?*/Zn (E°=-0.76V) and Cu2+/Cu (E°=0.34V).…

A: Electrolytes involved: Zn2+/Zn and Cu2+/Cu Mass of Zn reacting = 30 g Standard reduction potential…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe"(aq) +…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: Calculate the pH of the cathode compartment for the following reaction given Ecell = 3.01 V when…

A: We know that., PH  =  - log [H+]

Q: A cell consisting of a chromium strip and a lead wire, immersed in 1 M aqueous solutions of Cr(NO3)3…

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Q: current of 9.7 A and a voltage of 4.5V are used in the electroplating. How many grams of chromium…

A:

Q: 1) For the following combination of electrodes and solutions, indicate, 0.340 V a) Anode, cathode…

A: E° Cu2+/Cu is 0.34 V E° Ag+/Ag is 0.79 V Ag+ gets reduced and Cu gets Oxidised.

Q: For the galvanic (voltaic) cell Fe(s) + Mn2" (aq) Fe2*(aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A: We can use the Nernst equation to calculate the Ecell of a reaction. We have to get number of…

Q: For the cell diagram: Mg(s)|Mg2+(aq)|2H+(aq)|H2(g)|Pt(s) which reaction occurs at the anode?

A:

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…

Q: The Fe 2+ present in myoglobin (Mb) is oxidized by molecular oxygen (O2 ) in a process of 1 electron…

A:

Introduction to chemistry

Chemistry is a branch of science that deals with the analysis of material and the substances that comprise it. It also manages the properties of these substances and their reactions to form new substances. It is basically centered on particles and atoms that make up components and mixtures. These chemical species will in general connect using bonds.