+ ||ΣTRWhat would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions?H* = 0.76 MPH, = 2.7 atmT = 298 K10:25F4EゴF5F7F11F12PrtScrInsertDelete#3244.5.7.Backspace8.E.F.%3DK.C.B.

Answered: Image /qna-images/answer/a2a2c130-699a-45df-8bcd-71abcec85701.jpg

Answered: What would the potential of a standard…

What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions? H = 0.76 M PH, = 2.7 atm T = 298 K %3D E = V

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: Multiple Choice For each pair of standard cell potential and electron stoichiometry values below,…

Q: After plotting the cell potential (Ecell) measured at 298 K on the y-axis versus the natural…

A: Answer: Nernst equation for calculating cell potential is shown below: Ecell=Ecell0-RTnFlnQ Here:…

Q: For a given reaction associated with an electrochemical cell, K = 0.00134 and Q = 8.75. Use the…

A: The objective of the question is to determine the relationship between Eºcell and Ecell for a given…

Q: Saturated Ag/AgCl reference || Ti³+ (0.0850 M), Ti²+ (0.0450 M) || Pt

A: given E Ag/Agcl = 0.199v E; Ti+3/Ti+2 =-0.369V Ti+3=0.0850M Ti+2=0.0450M find Ecell

Q: 7. The potential observed in the cell diagrammed below (Ecell) is +0.290 V with the hydrogen…

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

Q: give proper explanation.

A: The objective of this question is to calculate the change in Gibbs free energy (ΔG°) for the given…

Q: Consider the electrolysis reactions cathode anode H₂O(1) whose standard reduction potentials can be…

A: According to the reaction,The reaction at the cathode can be written as,The reaction at the anode…

Q: For a galvanic cell, given the following half-reactions and their standard reduction potentials:…

A: The relation between Eocell and equilibrium constant is given as follows;logK=nEo0.0591 ----(1)

Q: A galvanic cell is constructed of two half cells Zn2+*(aq)/Zn(s) and H2(g)/H*(aq) separated by a…

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

Q: The Zn electrode is the

A: In cell notation left side written are anode half cell and right side of species after salt bridge…

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

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

A: Given: Molar concentration of [H+] is 0.83 M Pressure of H2 (PH2 ) is 3.1 atm Temperature T is…

Q: A hydrogen electrode is immersed in a 2.4 M solution of acetic acid at 25 °C. This electrode is…

Q: Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00207 M…

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

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

Q: Part A For the reaction what is the cell potential at 25°C if the concentrations are [Co³+] = 0.858…

Q: I what would be the potential of a standard hydrogen electrode (S.H.E.) be under the following…

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 2 (s) + 2 Br (aq) --> 21…

A: To find : E°cell = ? Formulae used : ∆G° = -nFE°cell ∆G° = - RT lnK Thus, -nFE°cell = - RT lnK…

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

Q: 4+ In a standard electrochemical cell, A is reduced to solid A, while gaseous Z2 is oxidized to Z³-.…

A: Given that, A4+ is reduced to solid A, i.e., A4+(aq) → A(s). Also, gaseous Z2 is oxidized to…

Q: Consider the following reaction Fe+3 + e- = Fe+2 E O = 0.771 When the potential of a platinum…

A: An electrochemical cell is a device that can generate electrical energy from the chemical reactions…

Q: 10. State the direction in which the reaction proceeds and calculate the cell potential for: 2Cr*…

A: The electrode potential is the ability of an electrode to lose or gain electrons is known as…

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 12 (s) + 2 Br (aq) --> 21…

A: Equilibrium constant (Kc) = 1.1 × 10-18 Temperature (T) = 298 k Standard cell potential (E°) = ? •…

Q: Calculate Cell Potential (Ecell) of the following galvanic cell, (E° cell = 1.10 V) Zn(s) | Zn²+…

Q: 3. Use a table of standard thermodynamic values to predict the standard cell potential at 71 C:…

A: Given cell notation is : Cu(s) | CuSO4 || AgNO3 | Ag (s) Use the standard thermodynamics values to…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

Q: A Ag|AgCl|CI electrode has an E= 0.197 V and a S.C.E has an E = 0.241 V. A redox species is measured…

A: The reference electrode, by convention, is used as the anode. The cell potential for the cell in…

Q: For a galvanic cell, given the following half-reactions and their standard reduction potentials:…

A: The galvanic (voltaic) cell is the cell in which the reaction takes place spontaneously. The…

Q: Determine the standard cell potential, E° cell, for a galvanic cell that employs the half-reactions…

A: Given: Reduction potential of MnO4-/Mn2+ half reaction is 1.506 V. Reduction potential of…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions?…

A: The potential of standard hydrogen electrode ( S.H.E ) can be calculated by using Nernst equation. E…

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

Q: Obtain the standard electrode potential and the Gibbs free energy of the reaction below: Fe(s) +…

A: We have to divide the cell reaction into two halve reactions. One is oxidation half and another is…

Q: Consider an electrochemical cell operating under standard conditions and at 25 °C. One half cell is…

Q: The value of pOH of HCI solution at 25 °C if cell potential of the cell is 1.6655 v Pt/ H2(g. 1.0…

A: The electrode where reduction process takes place is called cathode and where oxidation takes place…

Q: What is the cell potential, Ecell, at 298K for the following cell under non-standard conditions when…

Q: E = [H*] = 0.50 M PH₂ = = 3.9 atm T = 298 K

A: [H+] = 0.50M PH2 = 3.9 atm T = 298K

Q: Calculate the cell potential for the following electrochemical cell at 25°C. Sn(s) i Sn2+(aq, 0.022…

A: E°cell= E°(cathode)- E°(anode) [Sn^2+] = 0.022M [Ag^+] =2.7M

Q: Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard…

A: The process of breaking the electrolyte by applying an electric charge to its constituent ions is…

Q: Determine the Cell potential (volts, V) of a spontaneous galvanic cell rxn under the conditions; 2…

Q: For the reaction 2Co3+(aq)+2Cl(aq)->2Co2+(aq)+C12(g). Eocell=0.46 V what is the cell potential at 25…

A: Answer:Value of cell potential at 298.15K temperature is:Here:n is equal to number of electrons…

Q: Calculate the cell potential of each of the following electrochemical cell at 25oC. c. Pt|…

A: An electrochemical cell is a device which converts chemical energy to electrical energy from the…

Q: The potential of the following cell is -0.426 V. What is the K₂ for the generic acid RH? S.C.E.…

A: To find the Ka for the generic acid RH, we first need to identify the redox reaction occurring in…

Question

+ ||
Σ
T
R
What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions?
H* = 0.76 M
PH, = 2.7 atm
T = 298 K
10:25
F4
Eゴ
F5
F7
F11
F12
PrtScr
Insert
Delete
#3
24
4.
5.
7.
Backspace
8.
E.
F.
%3D
K.
C.
B.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

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

Calculate the potential of the cell when; [I- ] = 0.75 M, pH = 8.90, T = 300 K, P(H2 ) = 60 torr. Of course (R = 8.314 J/mol.K) and (F = 96500 J/V.mol). If E∘cell = -1.36v
From the following balanced redox reaction, determine the standard cell potential, the equilibrium constant and the standard Gibb's Free Energy at 298 K (3 sig. figs. for all). Do not include units in your answers and use the Electrode Reduction Potentials.pdf. tables. E°, = (0.0592) log(K) cell AGn = -nFE cell F = 96,485 C/mole e 5 Pb(s) + 2 MnO4 lag) + 16 H*ao) = 5 Pb2+ + 2 Mn2+ *fag) + 8 H2O) (ag) E°cell= V Keg = rxn kJ/mole
(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -). A spontaneous reaction has a negative Gibbs free energy change and a positive emf. A spontaneous reaction has a positive Gibbs free energy change and a negative emf. O Electron stoichiometry must be used to interconvert a Gibbs free energy change and a reaction emf. O A Gibbs free energy change involves coulombs of substances whereas an emf involves moles of electrons.
What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions? H*] = 0.70 M PH, = 2.6 atm T = 298 K V E =
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+] = 0.72 M PH₂ = 2.7 atm E = T = 298 K V
Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 What is the potential of the galvanic cell when In3+ is 0.023 M, In+ is 0.37 M, and U3+ is 0.076 M?
When [Pb2+] = 1.40 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.150 V. What is the Mn2+ concentration in this cell? Pb2*(aq) + Mn(s)– Pb(s) + Mn²+(aq) [Mn2+] = mol/L
Calculate the potential for each cell as written at 25 °C. Indicate whether the metal electrode in the half-reaction opposite the standard hydrogen electrode, S.H.E., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely. S.H.E. Zn2+(aq, 0.0600 M) Zn(s) E;, = -0.762 V Zn²+/Zn The Zn electrode is the .762 Ecell V cathode. Incorrect anode. Pt(s) V3+(aq, 0.215 M), V²+(aq, 0.00540 M) || S.H.E. = -0.255 V v3+/V2+ The Pt electrode is the .255 Ecell V cathode. Incorrect anode.
For the cell below, the standard potential is Eocell = 1.62 V ( F =96500 C/mole e-)( 1VC=1J) Mg(s) | Mg2+ (1M) || Zn 2+ (1M) | Zn (s)Calculate ΔGo for the cell at standard conditions in kJ. Select one: a. -1.62 kJ b. -313 kJ c. -3.13 x 105 kJ d. -156 kJ
Calculate the potential of the cell when; [I] = 0.75 M, pH = 8.90, T= 300 K, P(H2) = 60 torr. Of course (R = 8.314 J/mol.K) and (F = 96500 J/V.mol).
8:51 AM Mon Dec 5 = S BIOL 286 E B Lecture Pow... Bb Lecture Pow... O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free... cell A B A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. C Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. n 1 AA 1 1 Explanation 142. kJ/mol O calculated quantities (Check the box next to any that are wrong.) AG - 50. kJ/mol O - 46. kJ/mol O Check www-awu.aleks.com K 24 7.54 x 10 O…
Which of the following reaction is feasible? (Standard electrode potentials of Ca= -2.87V; Zn= -0.76V; Ba= -2.90V; Al= -1.66V; Pb= -0.13V; Mg= -2.37V; Cr= -0.74V; Cd= -0.40V) a. Pb + ZnsO4 + Zn PbSO4 O b. Al+ CrCl3 AICI3 + Cr Cdcl2 O c. Cd + CaCl2 - CdCl2 + Ca O d. Mg + BaCl2 - MgCl2 + Ba