Answered: For the galvanic cell at 298 K Zn(s) +…

For the galvanic cell at 298 K Zn(s) + 2 Ir2+(aq) → Zn2+(aq) + 2 Ir*(aq) Ecell = 0.36 V What is the equilibrium constant, K? Ecell = E° cell 0.0592 Flog Q in а. 1.5x1012 b. 13

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: Calculate the emf of a cell operating with the following reaction at 25°C, in which [MnO4-] = 0.010…

A: This problem is based on the Nernst equation which relates EMF of a cell with the concentration of…

Q: A voltaic cell is constructed with two Fe2+-Fe electrodes, where the half-reaction is…

A: Given that: E° = –0.45 V [Fe2+]oxd = 0.0088 M [Fe2+]red = 1.23 M T = 298 K To find: Ecell ?

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

A: The cell notation given is, Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣ Au3+(aq,? M) ∣ Au (s)

Q: Calculate the emf at 298 K generated by a voltaic cell in which the reaction isCr2O72-(aq)+ 14…

Q: Which reaction can take place spontaneously? TABLE: Standard Electrode (Reduction) Potentials at 25…

A: According to the given standard reduction potential, those species with less negative reduction…

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd2+ + 2 e Cd (a)…

Q: calculate the cell potential for the following reaction that takes place in an electrochemical cell…

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

Q: A galvanic cell is prepared using aluminum and nickel follows the cell notation Al(s) | AI3+(aq) ||…

Q: The value of K, for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br°(aq)…

A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq) E°=0.070 V The Ksp value 5.4×10-13

Q: What will be the overall balanced reaction if you want to make a galvanic cell? What is the…

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s) + 2 H+(aq) ⇔ Ni+2(aq) + H2 (g) Ecello = 0.23…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+. Initial concentrations: [Ni2+] =…

Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

Q: Consider a galvanic electrochemical cell constructed using Cr/Cr3* and Zn/Zn?+ at 25 °C. The…

A: The electrode with higher reduction potential of the metal is known as cathode. In this cathode,…

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: The objective of this question is to calculate the standard cell potential for a galvanic cell…

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: Given, AgCl s + e- → Ag s + Cl- aq E°red = 0.2223 V…

Q: Consider a galvanic cell that uses the reaction 2 Ag"(aq) + Sn(s) 2 Ag(s) + Sn2*(ac Calculate the…

A: Electrolytic cell that comprises of two half-cells with the same electrodes but have different…

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

Q: Calculate the standard cell potential, E°cell, for the following reaction, and indicate if the…

A: We are given a redox reaction happening in an electrochemical reaction. The oxidation half-reaction…

Q: What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2…

A: Given : half cell reaction Tip : cell having higher value of reduction potential will reduced

Q: Calculate the equilibrium constant, K at 25 °C for the reaction E cell = 1.53 V Zn2+ (aq) + 2 Fe2+…

A: We have to calculate the equilibrium constant for the given redox reaction.

Q: 5) Calculate the cell potential for the following reaction that takes place in an electrochemical…

Q: For the following electrochemical cell: Ag(s) | Ag+(aq) | | Fe2+(aq) | Fe(s) A. Calculate the Ecell…

A: To determine the deltaG° value , first we will determine the value E°Cell. The reaction between…

Q: concentration of Ae^+2 when Dw^+2 the cathode has

A: The net cell reaction, Ae + Dw2+ ------> Ae2+ + Dw E°cell = E°c - E°a = 2.108 - 2.156 =…

Q: - Part A - Compute the cell potential at 25 °Cunder the following conditions: [Sn+] – 1.68×10-2 mol…

A: We are given E° cell and we habe to find the Ecell

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: The objective of this question is to calculate the standard free energy for the reaction in the…

Q: A voltaic cell consists of a Pb/Pb²+ half-cell and a Cu/Cu²+ half-cell at 25 °C. The initial…

A: ECell can be calculated using nernst equation.

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: Given-> E°Ni2+/Ni = -0.25 V E°Co2+/Co = -0.28 V

Q: Determine the Ecell for the following reaction if the reaction contains 0.725 M Ni2+(aq) in one…

A: Given : cell reaction Tip : apply nernst equation

Q: Imagine an electrochemical cell established from the following half cells, linked by a KCI salt…

A: We have given that 1. a Fe electrode in 2.0M FeCl2 2. a Ni electrode in 2.0M Ni(NO3)3 Ni2+ +…

Q: Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s)…

A: E°cell indicates standard potential value but Ecell indicates potential value at given conditions.…

Q: voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following…

Q: hat is the standard cell potential of the following electrochemical cell at 25°C: i(s) | NiCl2(aq)…

A: Given-> Ni(s)/NiCl2(aq)//Cu(NO3)2(aq)/Cu(s)

Q: Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are…

A: Overall standard cell potential is calculated using this formula,E°cell=Ecathode-Eanode Balanced…

Q: Consider a galvanic cell that harnesses the free energy from the redox reaction below. MnO4-(aq) +…

A: Interpretation - For a given galvanic cell that harnesses the free energy from the redox reaction…

Q: The free energy change for the following reaction at 25 °C, when Cr³+ = 1.20 M and Zn²+ 2Cr³+ (1.20…

A: In the question, the reaction isWe need to find for this reaction. and

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential for the…

A: Given: K+(aq) + e- → K(s), E∘ = -2.93 V I2(s) + 2e- → 2I-(aq), E∘ = +0.54 V We have to find…

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: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: The Nernst equation is given as :

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

Q: A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e →…

A: Given that, for a galvanic cell, two half-cell reactions are NO3-aq + 4H+aq + 3e- → NOg + 2H2Ol…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

For the galvanic cell at 298 K
Zn(s) + 2 12+(aq) → Zn2+(aq) + 2 Ir*(aq)
E°cell = 0.36 V
What is the equilibrium constant, K?
Ecell = E° cell
0.0592
Flog Q
%3|
in
а.
1.5x1012
b.
6.8x10-13
С.
1.2x106
d.
8.3x10-7

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

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

4 Consider the voltaic cell: Sn(s) | Sn*2(aq) II Fe*3(aq) | Fe*2(aq) a) Write the overall cell reaction. b) Calculate the standard cell potential at 25°C. c) Calculate the change in free-energy of the reaction at 25°C d) What is the maximum work you can obtain from 25.0 g of nickel? e) What is the value of the equilibrium constant of the reaction? f) Which is the stronger oxidizing agent: Sn*2 or Fe*3? Explain
What is the potential of the reaction?
The redox reaction 3 Cl, (g) + 2 Al(s) → 2 Al³ † (aq) + 6 CI"(aq) consists of the two half-reactions shown. Cl, (g) + 2 e- –→ 2 Cl¯(aq) E. red = +1.36 V Al3 + (aq) + 3 e Al(s) Eed = -1.66 V What is the standard cell potential? 3.02 V 7.70 V -3.02 V O -0.30 V
For the galvanic (voltaic) cell Fe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²⁺] if [Mn²⁺] = 0.030 M and E = 0.78 V? Assume T is 298 K
Which statement is correct for the cell with a notation Pt /Cl2(g)/Cl¯(aq) // Zn+2(aq)/Zn ? choose 1 Neither of the anode and cathode is a standard hydrogen electrode. The cathode is a standard hydrogen electrode. The anode is a standard hydrogen electrode.
A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
A voltaic cell is constructed with two Ag+-Ag electrodes, where the half-reaction is Ag+(aq) + e– → Ag(s) E° = 0.80 V The concentrations of Ag+ ion in the two compartments are 0.023 M and 1.3 M. What is the cell potential at 25°C?. Explain
Consider the following electrochemical cell at 298 K where the source of Cu2+ (aq) is the sparingly soluble salt CuX. Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s) Zn2* + 2e = Zn E° = -0.76 V Cu2+ + 2e = Cu E° = 0.34 V If the potential created from this cell = 1.03 V, what is Ksp for CuX? O 1.9x10-9 3.8x10 12 4.6x10 6 2.0x10 7
10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V с. 0.60 V d. -0.60 V e. 0.095 V enstant fr ther
The standard cell potential E° cell for the voltaic cell based on the reaction below is V. 3 Sn 4+ (aq) + 2 Cr(s) - 2 Cr 3+ (aq) + 3 Sn 2+ (aq) 2 e- + Sn 4+ (aq) Sn 2+ E° red = +0.154 V - (aq) 3 e- + Cr 3+, (aq) CI(s) E red = - 0.74 V (answer has no unit)