A prod01-cnow-owl.cengagenow.comBb ContentX OWLV2 | Online teParaphrasing ...ewriting ToolCar noteCAU EMAILCANVASPirate ShipMYJSCCBLACKBOARD[References]Use the References to access important values if nConsider the following cell reaction:Zn(s) + 2 H*(? M) –Zn²*(1.00 M) + H2(g)(1.00 atm)If the cell potential at 298 K is 0.201 volts, what is the pH of the hydrogen electrode?pH =Submit AnswerTry Another Version3 item attempts remainingDEC 310étv Nali 1

Answered: Image /qna-images/answer/2614f8e2-6278-4ad7-975e-31256881e49c.jpg

Consider the following cell reacțion: Zn(s) + 2 H*(? M) Zn2*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.201 volts, what is the pH of the hydrogen electrode? pH =

Consider the following cell reacțion: Zn(s) + 2 H(? M) Zn2(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.201 volts, what is the pH of the hydrogen electrode? pH =

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.19QAP

See similar textbooks

Related questions

Q: Consider the following cell reaction: Co(s)+2 H (? M) Co2*(1.00 M)+ H2(g)(1.00 atm) If the cell…

A: The pH of the acid solution is less than 7 and while of the base is greater than 7. The pH and…

Q: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction: 2X(s) + 3Y2+(aq) →2X3+ + 3Y(s) As the charges are equal on both sides.…

Q: For the cell reaction, Zn(s) | Zn2+(aq, 1 M) || Cu2+(aq, 1 M) | Cu(s), the electrode potential of…

A: In the given question we have to calculate the cell potential. cell Reaction, Zn(s) + Cu2+(aq)…

Q: Use the Nernst equation to calculate the cell potential, Ecell , for a galvanic cell consisting of…

Q: What is the initial cell potential? Express your answer to two decimal places and include the…

A: Initial concentration of Ni2+ = 1.80 mol/L Initial concentration of Zn2+ = 0.120 mol/L The…

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18.0 h.If…

A: According to Faraday's first law, when a certain amount of current flows through an electrolyte, the…

Q: The standard reduction potential of the Pb2+/Pb electrode is -0.13 V and the standard cell potential…

Q: (a) Balance the following simple redox reaction. Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4 OH- (3) (b) If…

A: Redox reaction : it is the reaction where oxidation and reduction are occurred simultaneously . the…

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M)→FE²*(1.00 M)+ H2(g)(1.00 atm) - If the cell…

A: Given: A cell reaction: Fes + 2H+?M → Fe2+1.00M + H2g1.00atm Temperature = 298K Cell potential =…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* 1.0 M…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: The cell potential for the standard galvanic cell shown above is +1.56V. If AgNO3(aq)|Ag(s) is…

A: Initially, At cathode: E°AgNO3/Ag=+0.80 V (reduction)At anode : E°Zn(NO3)2/Zn=-0.76 V…

Q: Your mystery voltaic cell has a standard cell potential of 0.741 V and can be written in cell…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: The standard cell potential for the reaction provided below is 0.301 V, (where X is a non-metal…

A: Interpretation - To determine the cell potential when there are 14.6 g of X, PH2 = 2.99atm, and…

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M)-Mn2+(1.00 M) + H₂(g)(1.00 atm) If the cell…

Q: The standard cell potential for the reaction provided below is-2.431V, calculate the cell potential…

Q: Devise cells in which the following are the reactions and calculate the standard cell potential in…

Q: Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg−1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) Fe2*(1.00 M) + H2(g)(1.00 atm) If the cell…

A: By applying formula Ecell = E•cell - 0.0591/2 . Log[Fe2+]| [H+]2 At 25 degree Celsius

Q: Given that the standard electrode potentials (E°) of metals are :K+/K = -2.93 V, Ag+/Ag = 0.80 V,…

A: Lower the value of reduction potential, stronger the reducing agent and higher the value of…

Q: Consider the following equation, if the cell potential is 1.136 V at 25∘ C, determine the standard…

Q: A fuel cell is constructed in which both electrodes make use of the oxidation of methane. The…

A: (a)

Q: A galvanic cell consists of a Mg electrode in 1 M Mg(NO3)2 solution and a Ag electrode in 1 M AgNO3…

A: Given- Electrodes Mg in 1 M Mg(NO3)2 solution Ag in 1 M AgNO3 solution Temperature = 25 °C To…

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Given data : Mn(s) + 2 H+(_____M) gives Mn2+(1.00 M) + H2(g)(1.00 atm)the cell potential (E cell…

Q: The standard cell potential of a voltaic cell consdtructed using the cell reaction below is 0.772 V.…

Q: For the standard cell potentials given here, determine the ΔG° for the cell in kJ.(a) 0.000 V, n =…

Q: An inventor proposes using a SHE (standard hydrogen electrode) in a new battery for smartphones that…

Q: 1. (a) Balance the following simple redox reaction. Fe (s) + O2(g) + 2H2O (I) → Fe3* + 4 OH (b) If…

A: In an electrochemical reaction redox reaction occur in different electrode At cathode we expect…

Q: Gibbs energy change, A;G°, is related to cell potential, Eel, by the equation A;G° = -nFEl Part B…

A: The given reaction is as follows: Xs+2Y+(aq) → X2+(aq) + 2Y(s) ∆rG° of the reaction can be…

Q: Consider the following reaction with vanadium and iron: 2 Fe2+ (aq) + √2+ (aq) 2 Fe³+ (aq) + V(s)…

A: Here we have to predict the Ecell at equilibrium of the following given cell reaction.

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) –→FE²*(1.00 M) + H2(g)(1.00 atm) If the cell…

Q: Consider the following electrochemical cell notation with a cell potential of 0.300 V. Pt ∣Cr3+(aq,…

A: NOTE : There is a minor correction in the cell notation given. As per the rules, the specie which is…

Q: Consider the following cell reaction: Ni(s) + 2 H+(? M) Ni2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) –→MN2*(1.00 M) + H2(g)(1.00 atm) If the cell…

Q: alculate the standard potential, ?∘, for this reaction from its Δ⁢G° value.…

A: Standard Reduction Potential - It is the difference between the reduction potential of cathode and…

Q: Consider the following cell reaction: Co(s) + 2 H*(? M) Co2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Here we are required to find the pH of hydrogen electrode

Q: Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn (s) + Cu²*…

Q: The cell shown below has a measured cell potential of +0.06839 V at 25.0 °C. A graph of the cell…

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: Given reaction is : 2Ag+ (aq) + Cu (s) ------------> 2Ag (s) + Cu2+ (aq) , ΔG0 = -88660 J/mole…

Q: 11. Consider the following reaction and its AG-AG• at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: For given reaction and given ∆G° value , E°cell and K can be calculated using relations with ∆G° .

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) –Fe²*(1.00 M) + H>(g)(1.00 atm) If the cell…

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) Fe"(1.00 M) + H2(g)(1.00 atm) 2+ If the cell…

A: We wil first write nernst equation, and then calculate pH of solution.

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) Mn2*(1.00 M) + H2(g)(1.00 atm) If the cell…

A: According to the given cell reaction, Mn is being oxidized to Mn2+ and hydrogen ions are being…

Q: Consider the following reactions. Are they spontaneous in the direction written, under standard…

A: Cell with positive EMF represents negative free energy change with accompanies spontaneous change.

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) "(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Since you have asked multiple question, we will solve the first question for you as per our…

Q: How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis W= (E×i×t)/96500 W= mass of a…

Q: Use the biological standard potentials of two reduction reactions 4H* + 4e + 02-> 2 H20, E = + 0.82…

Q: Cu"taa) Sn (aa) Cus Consider a cell: Sn in which the concentration of [Cu2*] and (Sn2] are both 2M.…

Q: Consider the following cell reaction: Ni(s) + 2 H*(? M) →Ni²*(1.00 M) + H2(g)(1.00 atm) If the cell…

Question

A prod01-cnow-owl.cengagenow.com
Bb Content
X OWLV2 | Online te
Paraphrasing ...ewriting Tool
Car note
CAU EMAIL
CANVAS
Pirate Ship
MYJSCC
BLACKBOARD
[References]
Use the References to access important values if n
Consider the following cell reaction:
Zn(s) + 2 H*(? M) –Zn²*(1.00 M) + H2(g)(1.00 atm)
If the cell potential at 298 K is 0.201 volts, what is the pH of the hydrogen electrode?
pH =
Submit Answer
Try Another Version
3 item attempts remaining
DEC 3
10
étv Nali 1

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

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.
Why is a salt bridge necessary in galvanic cells like the one in Figure 17.4?
Use the following half-equations to write three spontaneous reactions. Justify your answers by calculating E° for the cells. 1. MnO4(aq)+8H+(aq)+5eMn2+(aq)+4H2OE=+1.512V 2. O2(g)+4H+(aq)+4e2H2OE=+1.229V 3. Co2+(aq)+2eCo(s)E=0.282V
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
Consider a cell reaction at 25°C where n=2 . Fill in the following table.
Consider a cell reaction at 25°C where n=4 . Fill in the following table.
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?
Calculate E° for the following cells: (a) Ag|Ag+Sn4+,Sn2+|Pt (b) Al|Al3+Cu2+|Cu (c) Pt|Fe2+,Fe3+MnO4,Mn2+|Pt
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.