When the Cu2+ concentration is 9.50x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.985V. What is the Cr3+ concentration? 3Cu²+ (aq) + 2Cr(s)-3Cu(s) + 2Cr³+ (aq) Answer: M

When the Cu2+ concentration is 9.50x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.985V. What is the Cr3+ concentration? 3Cu²+ (aq) + 2Cr(s)-3Cu(s) + 2Cr³+ (aq) Answer: M

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 111AE: The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making...

See similar textbooks

Related questions

Q: When the Cu2+ concentration is 9.20x10-4 M, the observed cell potential at 298K for an…

A: A question based on batteries. Using the given data, the concentration of Al3+ is to be calculated.

Q: When the Hg2+ concentration is 2.39×10-4 M, the observed cell potential at 298K for an…

A: The given redox reaction is Hg2+(aq) + Zn(s)→ Hg(l) + Zn2+(aq) The concentrations of the species are…

Q: When the Ag + concentration is 1.05 M, the observed cell potential at 298K for an electrochemical…

Q: When the Cu2+ concentration is 1.47 M, the observed cell potential at 298K for an electrochemical…

Q: When the Pb2+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical…

Q: When the Pb2+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical…

Q: When the Hg2+ concentration is 4.61×10-4 M, the observed cell potential at 298K for an…

A: Given:The given electrochemical cell isCalculate the concentration.Cell potential, is denoted as ,…

Q: When the Pb2+ concentration is 1.10 M, the observed cell potential at 298K for an electrochemical…

Q: When the Pb2+ concentration is 5.46×10-4 M, the observed cell potential at 298K for an…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: When the Ag* concentration is 1.25×104 M, the observed cell potential at 298K for an electrochemical…

Q: When the Cu²+ concentration is 9.81x10-4 M, the observed cell potential at 298K for an…

A: Given, Cu2+(aq) + Mn(s) ---> Cu(s) + Mn2+(aq) Cell potential (Ecell) = 1.428 V [Cu2+] = 9.81 ×…

Q: When the Hg2+ concentration is 1.22×104 M, the observed cell potential at 298K for an…

A: It is given that Ecell for the given cell is 1.477V at 25°C and the concentration of Hg2+ is 1.22×10…

Q: When the Pb²+ concentration is 1.49×104 M, the observed cell potential at 298K for an…

A: Given,The cell reactions:(i) cell potential = 0.501 V[ Pb2+ ] = 1.49 x 10-4 M

Q: 6) Given the table below predict the numerical value of the standard cell potential for the…

Q: Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the…

A: Step1:Explanation:A redox reaction involves electron transfer between substances, where one is…

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

Q: When the Hg2+ concentration is 1.16 M, the observed cell potential at 298K for an electrochemical…

A: The given electrochemical cell is 3Hg2+(aq) + 2Al(s)→3Hg(l) + 2Al3+(aq) Which is can be obtained…

Q: When the Cu2* concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

Q: When the Ag* concentration is 6.04×104 M, the observed cell potential at 298K for an electrochemical…

A: Given: Concentration of Ag+ = 6.04×10-4 M T = 298 K Ecell = 2.267 V Known: Standard reduction…

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

A: Given,

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

Q: When the Ag+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

A: The given cell is an electrochemical cell.

Q: When the Cu²+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

Q: When the Cu²+ concentration is 1.00 M, the observed cell potential at 298K for an electrochemical…

A: The given reaction is : The half reactions are : At cathode :Cu2+ + 2e- → Cu E°=+0.34 V…

Q: When the Hg2+ concentration is 1.07 M, the observed cell potential at 298K for an electrochemical…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

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

Q: When the Hg2+ concentration is 1.63×104 M, the observed cell potential at 298K for an…

A: To find the concentration of Al3+ in the given electrochemical cell, we will use the Nernst equation…

Q: When the Hg* concentration is 8.47x10+M, the observed cell potential at 298K for an electrochemical…

A: Formula used :- Ecell = E°cell - (2.303RT÷nF ) log([product]÷[Reactant]) At Room temperature…

Q: When the Hg2+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

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

Question

When the Cu2+ concentration is 9.50x10-4 M, the observed cell
potential at 298K for an electrochemical cell with the following
reaction is 0.985V. What is the Cr³+ concentration?
3Cu²+ (aq) + 2Cr(s)-3Cu(s) + 2Cr³+ (aq)
Answer:
M

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Calculate the theoretical potential of each of the following cells. Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Pt|Cr3+(2.00 10-4M),Cr2+(1.50 10-3 M)||Pb2+ (5.60 0215 10-2M)|Pb (b) Hg|Hg22+(2.00 10-2 M)||H+(1.50 10-2 M),V3+ (2.00 10-2M),VO2+(3.00 10-3M)|Pt (e) Pt|Fe3+(3.00 10-2 M), Fe2+ (4.00 10-5M)||Sn2+ (3.50 10-2M), Sn4+ (5.50 10-4 M)|Pt
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
Which of the changes below will increase the voltage of the following cell? Co|Co2+(0.010M)H+(0.010M)|H2(0.500atm)|Pt (a) Increase the volume of COCl2 solution from 100 mL to 300 mL. (b) Increase [H+] from 0.010 M to 0.500 M. (c) Increase the pressure of H2 from 0.500 atm to 1 atm. (d) Increase the mass of the Co electrode from 15 g to 25 g. (e) Increase [CO2+] from 0.010 M to 0.500 M.
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
What is wrong with the following statement: The best concentration cell will consist of the substance having the most positive standard reduction potential. What drives a concentration cell to produce a large voltage?
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+, 1.0 M Au3+, and 1.0 M NiH2+ in the cathode compartment of an electrolytic cell. Predict the order in which the metals will plate out as the voltage is gradually increased.
Calculate E° for the following cells: (a) Ag|Ag+Sn4+,Sn2+|Pt (b) Al|Al3+Cu2+|Cu (c) Pt|Fe2+,Fe3+MnO4,Mn2+|Pt
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?