The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the cell Zn(s) | Zn2+ (aq) || H+ (aq, 1 M) | H₂ (g, 1 bar) | Pt(s) is 0.81V at 25°C. What is the concentration of Zn²+ (aq) (in mol L-¹) ? 0 2 O 0.1 0.02 04 07

The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the cell Zn(s) | Zn2+ (aq) || H+ (aq, 1 M) | H₂ (g, 1 bar) | Pt(s) is 0.81V at 25°C. What is the concentration of Zn²+ (aq) (in mol L-¹) ? 0 2 O 0.1 0.02 04 07

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 equilibrium constant K for the overall reaction that takes place in the cell Pt|Sn2+,…

Q: Consider the cell: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) |…

Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A: In this electrochemical cell of cobalt metal acts as a anode and silver metal is acts as a cathode.…

Q: In the standard electrochemical cell, Pt(s)|H2SO3laq), H*(aq), SO4 (aq)||Ag*(aq)|Ag(s), v¥hat can be…

A: In a electrochemical cell representation RHS is cathode s reduction all happen over there, LHS in…

Q: Consider the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). The measured Ecell for…

A: Given that, the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). So, [Cu2+] = 0.1 M,…

Q: For the electrochemical cell Ni(s) | Ni 2+(1 M) || H +(1 M) | H 2(1 atm) | Pt(s), which one of the…

A: Well, cell reaction of Ni(s) | Ni 2+(1 M) || H +(1 M) | H 2(1 atm) | Pt(s) Anode- Ni(s)→Ni2+(aq)+2e…

Q: What are the overall cell reaction and the cell potential for this voltaic cell? Mg(s)|Mg (aq) ||…

A: Standard reduction potential of Mg2+|Mg = -2.38 V Standard reduction potential of Pb2+| Pb = -0.13 V

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: 12. A concentration cell consists of two hydrogen electrodes: Pt(s) | H2(g, 1 bar) | H+(aq, pH = ?)…

A: The standard electrode potential is zero for the concentration cell because the same substance gets…

Q: Write the individual electrode reactions and the overall cell reaction for the following cell: Pt |…

A: The electromotive force of the cell or of the EMF of the cell is the maximum potential difference…

Q: Calculate the standard Gibbs energy in kJ/mol change for the following voltaic cell A(s) | A3+(aq)…

Q: An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid…

A: First, we need to identify the reactions occurring at the anode and cathode. The hydrogen electrode…

Q: What is E at 25 °C fc

A: Electromotive force (EMF) of an electrochemical cell is a measure of the voltage or electrical…

Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C. Pt(s) |…

Q: An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid…

A: First, we need to identify the reactions occurring at the anode and cathode. The hydrogen electrode…

Q: The standard cell potential of a Daniell cell, with cell reactionZn(s) + Cu2+(aq) → Zn2+(aq) +…

A: Given, a Daniell cell with the cell reaction as follows,Zn(s)+Cu2+→Zn2++Cu(s)the standard cell…

Q: The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s)…

A: The cell diagram for the reaction is (-) Zn(s) | ZnO(s) | KOH(aq) || Ag2O(s) | Ag(s) (+) The…

Q: Calculate the concentration of Ag+ required to drop the cell potential to 0. Pt | Fe2+ (0.24…

Q: Write a balanced chemical equation for the overall cell reaction represented as (a) Ag|Ag* ||Sn*+ ,…

A: A balanced chemical equation for the given cell reaction needs to be determined.

Q: The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the…

Q: The cell reaction NiO₂ (s) + 4H+ (aq) + 2Ag(s)- Ni²+ (aq) + 2H₂O + 2Ag+ (aq) has Eºcell = 2.48 V.…

A: Given -> E°cell = 2.48 V pH = 2.00 [NI2+] = [ Ag+] = 0.030 M

Q: What is undergoing oxidation in the redox reaction represented by the following cell notation?…

Q: 8. Suppose that the concentrations of NaF and KCI were each 0.10 M in the cell Pb(s) PbF₂(s)…

A: 2. Recall the given cell representation, Pb s | PbF2 s | F- aq || Cl- aq |…

Q: A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn…

Q: Payalben

A: The objective of the question is to calculate the Gibbs free energy change and the maximum amount of…

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

Q: The potential of the cell Ag|AgI (s)| AgI (aq) |Ag is 0.9509V at 25C. Calculate the solubility of…

A: The half cell reactions of the Ag|AgI (s)| AgI (aq) |Ag cell are, Anode: Ag+I-→AgI++e-Cathode:…

Q: For the cell shown, the measured cell potential, Ecel, is-0.3621 V at 25 °C. Pt(s) | H, (g,0.853…

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

The standard reduction potential of the zinc cation is -0.76 V. The measured cell
potential for the cell Zn(s) | Zn2+ (aq) || H+ (aq, 1 M) | H₂ (g, 1 bar) | Pt(s) is 0.81V at
25°C. What is the concentration of Zn²+ (aq) (in mol L-¹) ?
0 2
O 0.1
0.02
04
07

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

9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?
Devise cells in which the following are the reactions and calculate the standard cell potential in each case. a. 2 Na(s) + 2 H2O (l) ---------> 2 NaOH(aq) + H2(g) b. H2(g) + I2(g) ---------->. 2 HI (aq) c. H3O+(aq) + OH-(aq) --------->. 2 H2O(l)
Determine the cell potential for the following cell Zn(s) | Zn2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Zn2+(aq) and Ag+(aq) are –0.76 V and +0.80 V, respectively. A. 1.45 V B. 1.67 V C. 1.56 V D. 1.51 V E. 1.61 V
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.
For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M), Cr2+(aq)(.301M)|Pt(s) Determine the cell potential for this electrochemical cell by first calculating the standard cell potential and then by using the Nernst equation.
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V
The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E') is 0.222 V at 25°C? Agls) | AgCl(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) O 6.1x 102 M O 3.7 x 103M O 4.9x 105 M
2. Calculate the cell potential for the cell below at 25 °C Ti(s) Ti(NO3)2(aq) (0.92 M)|| HgCl₂(aq) (0.43 M)|Hg(1)|