Xe"(aq) II Y3+ELECTROCHEMISTRY:Pt(s) IX*(a0), X2+,Given the line notation:(aq) || y3+,*(aq) | Y(s)where:x2+ + e - x+E° = 0.44 Vy3+ + 3 e - YE° = -1.99 VPt4+ + 4 e → PtE° = 1.20 VCalculate the EMF.

Answered: Image /qna-images/answer/6be60247-ad17-4d4b-9ab6-c2c74e851405.jpg

ELECTROCHEMISTRY: Given the line notation: Pt(s) |X*(aq)- x2+ (aq) || Y3+ *(aq) I Y(s) where: x2+ + e" - x* E° = 0.44 V y3+ + 3 e - Y E° = -1.99 V Pr4+ + 4 e → Pt E° = 1.20 V Calculate the EMF.

ELECTROCHEMISTRY: Given the line notation: Pt(s) |X(aq)- x2+ (aq) || Y3+ (aq) I Y(s) where: x2+ + e" - x* E° = 0.44 V y3+ + 3 e - Y E° = -1.99 V Pr4+ + 4 e → Pt E° = 1.20 V Calculate the EMF.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The following potential diagram summarizes the results of electrochemical studies of the aqueous…

A: The reduction potential of ClO4- to Cl2 will be the change of total reduction potential of every…

Q: Balance the following reaction under acidic conditions and calculate cell potential at 298K Cr2O72-…

A: Calculate cell potential Using Nerenst equation

Q: The E° cell 0.135 V for the reaction B1,(s) + 5Cr20,2(aq)+ 34H (aq) – 6103 (aq) + 10Cr+(aq) + 17H20…

A: 1st we balanced the equation to find out what number of electrons involved in this reaction. then we…

Q: A galvanic cell is constructed in which the overall reactionis Cr,0; (aq) + 14 H2O* (aq) + 6I¯ (aq)…

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

Q: The standard addition method is used to determine the concentration of vitamin C in apple juice by…

A: Given : Initial volume of sample of apple juice = 2.00 mL Final diluted volume of apple juice = 25.0…

Q: Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure…

A: This problem is related to Faraday`s Law of electrolysis, states as "mass of substance deposited or…

Q: 2Cr3+(aq) + 3Ni(s) Eocell = 0.51 V What is the measured cell potential (Ecell) when…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu2+(aq) +…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cr³+ (aq)…

Q: ELECTROCHEMISTRY Write the redox reactions and calculate the standard e.m.f.: Ce3+(aq) | Ce4+(aq)…

Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

A: An electrolytic cell is a cell which requires an outside electrical source to initiate the redox…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀…

Q: (i) Pt(s) + 2 NH3(aq) + 2 CI ( (aq) cis-[PtCl₂(NH3)2](aq) + 2 e¯ E° = 0.274 V The likely cathodic…

Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

A: Concept- By the help of nernst equation, this problem can be solved. Ecell=Eocell− 0.0592/n log10Q…

Q: Calculate the standard potential, Eº, for this reaction from its equilibrium constant at 298 K. X(s)…

Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

A: Let voltage required is V volt . And we are given 91%effeicient current = 6.82 ,so nett effective…

Q: Calculate the cell potential for the reaction: 2Fe3+ + 2I− → 2Fe2+ + I2 from the reduction…

A: In a Galvanic cell , oxidation takes place at anode and reduction takes place at cathode If…

Q: ELECTROCHEMISTRY: Pt(s) |X*(ag), X2 *(aq) || Y3*(aq) | Y(s) Given the line notation: where: x2+ + e…

Q: A galvanic cell is constructed in which the overall reac- tion is Brz (€) + H2(g) + 2 H20(€) → 2 Br…

A: ∆E∘ is calculated from the standard reduction potential values: ∆E∘=Ecathode∘-Eanode∘ In this…

Q: The cell SCE // Ag2CrO4 (sat'd), CrO42- (x M) / Ag is used for the determination of pCrO4. Calculate…

A: For the cell SCE // Ag2CrO4 (sat'd), CrO42-/ Ag, the reduction equation for silver chromate…

Q: The following cell was employed for the determination of pCrO4: SCE // CrO4 2-(xM) / Ag2CrO4 (s) /…

Q: For Ag+(aq) + e-→ Ag(s), Eº = +0.80 V and for Zn²+(aq) + 2e¯ → Zn(s), E° = -0.76 V. a) Identify…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Explain why the cell potential of the galvanic cells in this experiment decreases over time. Part A…

A: As we analyze the data we see that in each case the voltage of the galvanic cell decreases as we use…

Q: Pt(s) Br (aq) (x M) | Br21) || BrO3¯(aq) (0.43 M), H*(aq) (1.00 M) | Br2(1) | Pt(s)

Q: Calculate the cell potential in volts for following cell. Eo = +1.93 V Mg|Mg2+, 1.00 x 10-3 M||Fe2+…

Q: Calculate the time required to precipitate 200 milligrams of copper by electrolysis of an acidic…

A: By 1F of charge 1 equivalent of metal can be deposited .

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E"…

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 2.50 hr in an electrolytic cell…

A: According to Faraday’s first law, the chemical deposition which takes place during electrolysis is…

Q: Calculate the equilibrium constant, Keq, at 25 °C for the reaction: 2Br (aq) + I2 (s) Br2 (1) + 21-…

A: 2Br^-(aq) + I2(s)-->> Br2(I) +2I^-(aq) E°red(cathode)=0.54V E°red(anode)=1.066V

Q: Purification of chromium can be achieved by electrorefining chromium from an impure chromium anode…

A: The reaction taking place can be written as Cr3+ (aq) + 3 e- -------> Cr (s) Given : current =…

Q: 瓦,可 212 106% Q 6: Galvanic cell presented as Fe/Fe2 //Co²/Co, If reduction potential of iron = -…

Q: Calculate the equilibrium molarity of C2O4^2-

A: Given data:

Q: QI: Electrical cell fill by 0.1 M aqueous NaOH when pass( 3.5 A) through (9 hr) the conductivity of…

A: Solution -

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

Q: A Cu electrode is immersed in a solution that is 1.00 M in [Cu(NH3)4]2+ and 1.00 M in NH3. When the…

Q: What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the…

A: Answer:- This question is answered by using the simple concept of electrolysis which involves the…

Q: For ferricyanide determination by voltammetry, 20 mL of non-electroactive KCl solution is added to…

A: Molarity = No of moles / Volume (L) Also, No of moles = Molarity * Volume (L)

Q: Given the cell notation Pt /Cl2(g)/Cl¯(aq) // Zn+2(aq)/Zn. How long, in seconds, will it take for…

A: Given-> Weight of Zn =1.000 gm Atomic mass of Zn = 65.38 gm Current (i) = 2.000 ampere

Q: ELECTROCHEMISTRY: Given the line notation: Pt|Xa), X7+ (ag) Where: x2+ + e → X+ y3+ + 3e → Y Pt++ +…

Q: A galvanic cell is constructed in which the overall reac- tion is Cr,O (aq) + 14 H,0 (aq) + 61 (aq)…

A: GALVANIC CELL A galvanic cell is an electrochemical cell that converts chemical energy into…

Q: Given the following half-reactions and their standard reduction potentials, 2CIO;- + 12H* + 10e Cl,+…

A: E0ClO32- =1.47 V E0S2O82- = 2.01 V E0 cell = E0S2O82- -E0ClO32- = 2.01 - 1.47 = 0.54 V

Q: Given the following electrode reactions: 2+ Co +e Co“ E'=1,92 V 3+ Co(NH,) , +e Co(NH,), E-0,06 a.…

Q: A galvanic cell is constructed in which the overall reac- tion is Cr,O} (aq) + 14 H¿O*(aq) + 6 I…

A: Reduction half reaction: Cr2O72- + 6e = Cr3+ [E0 (Cr2O72-/Cr3+) = 1.33 V] Oxidation half…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: I₂ (s) +…

A: Equilibrium constant of a reaction is related to the emf of a cell which is related to the Gibbs…

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

A: Before solving this question we must knowthe folowing concept.suppose an equilibrium reaction :-A(g)…

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

Q: How many hours does it take to form 15.0 L of O2 measured at 750 torr and 30°C from water by passing…

A: According to Faraday's first law ,when current is passed through an electrolytic solution, the…

Q: A glass electrode dipped in a solution of 7 pH acidity was found to have a voltage of E = 0.395 V,…

A: The formula used to calculate the pH with glass electrode is as follows: Ecell = Eo + (0.0592 × pH)…

Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

Xe"(aq) II Y3+
ELECTROCHEMISTRY:
Pt(s) IX*(a0), X2+,
Given the line notation:
(aq) || y3+,
*(aq) | Y(s)
where:
x2+ + e - x+
E° = 0.44 V
y3+ + 3 e - Y
E° = -1.99 V
Pt4+ + 4 e → Pt
E° = 1.20 V
Calculate the EMF.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Pt(s) |X' (aq), X2+, ELECTROCHEMISTRY: Pt(s) |X* (aq). (aq) || Y3+, *(aq) | Y(s) Given the line notation: where: 2+ + e° x+ E° = 0.48 V y3+ + 3 e → Y E° = -2.4 V Pt4+ + 4 e - Pt E° = 1.20 V Calculate the EMF.
ELECTROCHEMISTRY: X2+ (aq) || Y3+ Given the line notation: Pt(s) |X* (aq). (aq) | Y(s) where: x2+ + e EO = 0.59 V y3+ + 3 e - Y E° = -2.21 V P4+ + 4 e → Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign
ELECTROCHEMISTRY: x2+ (aq) || Y3+ Given the line notation: Pt(s) |X*(ag). (aq) IY(s) where: x2+ + e - x* E° = 0.47 V y3+ + 3 e - Y E° = -2.65 V Pt4+ + 4 e E° = 1.20 V - Pt %3D Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign
Pt(s) |X ELECTROCHEMISTRY: Pt(s) |X"(aq). X2+ (aq)I/ Y3+ Given the line notation: (aq) I Y(s) where: x2+ + e x+ E° = 0.85 V -> y3+ + 3 e → Y E° = -2.44 V P4+ + 4 e - Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign
ELECTROCHEMISTRY: Given the line notation: Pts) |X*(aq) : (aq) || y3+ (aq) | Y(s) where: x2* +e - x* E° = 1.17 V y3+ +3 e - Y E° = -2.16 V Prt+ + 4e - Pt E° = 1.20 V Calculate the EMF.
ELECTROCHEMISTRY: Pt(s) |X* (aq) (aq) || Y3+ "(aq) | Y(s) Given the line notation: where: x2+ + e , x+ E° = 0.88 V y3+ + 3 e → Y E° = -2.46 V P4+ + 4 e -→ Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.
For the dissociation of iodic acid, HIO3(aq) + H20(1) H3O*(aq) + I03 (aq) If, at equilibrium, [HIO3(aq)] = 0.16 mol L-1, [H30*(aq)] = 0.29 mol L-1, and [103 (aq)] = 0.21 mol L1, calculate Ko. (Give 2 significant figures in your answer.) Answer:
ELECTROCHEMISTRY: Pt(s) |X" (aq). (aq) | Y(s) Given the line notation: (aq) || y3+ where: x2* + e x* E° = 0.48 V y3+ + 3 e → Y E° = -2.35 V Pt4+ + 4 e - E° = 1.20 V - Pt Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign
How long would it take (in minutes) to reduce 1 mole of each of the following ions using the current indicated? (Ampere (A) = Coulomb/second (C/s), I = C/s, F= 96500 C/mol e-) (C = Charge unit Coulomb, n = electron mole number) Q=I×t=n×F(a) Fe3+ , 2.344 A (b) Cu2+ , 25.260 A
Standard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s)…