When the Hg2+ concentration is 2.22×10-4 M, the observed cell potential at 298K for an electrochemical cell with thefollowing reaction is 1.486V. What is the Cr³+concentration?3Hg²*(aq) + 2Cr(s)3Hg(1) + 2C1³*(aq)Answer:M

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Answered: When the Hg2+ concentration is…

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...

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When the Agt concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.667V. What is the Zn2+ concentration? 2Ag+(aq) + Zn(s)2Ag(s) + Zn2+(aq) Answer: M
Can you please answer these two sub problems and show all of the steps to the solution
When the Ag* concentration is 2.63×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.324V. What is the Cr³+ concentration? 3Ag*(aq) + Cr(s)- →3Ag(s) + Cr³+ (aq) Answer: M
When the Cu2+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.610V. What is the Mn2+ concentration? 2+ Cu²*(aq) + Mn(s)→ Cu(s) + Mn²*(aq) Answer: M
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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 2.22×10-3 atm, the H† concentration is 1.38M, and the Cr3+ concentration is 3.60×10-4M ? 6.00H*(aq) + 2Cr(s)→3H2(g) + 2C1³*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
4
Zn(s) │ Zn2+(aq, 0.10 M) ║ Zn2+(aq, 0.50 M) │ Zn(s) The concentration cell above was allowed to operate until the cell reaction reached equilibrium. What are the cell potential and the concentrations of zinc(II) in each half-cell for the cell now?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s)+Cu2+(aq)⟶Cu(s)+Zn2+(aq)Zn(s)+CuX2+(aq)⟶Cu(s)+ZnX2+(aq) Eocell=1.1032 VEcello=1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn2+(aq)ZnX2+(aq) and 0.1701 M solution of Cu2+(aq)CuX2+(aq) at 441.2 K?
When the Ag+ concentration is 4.19×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.257V. What is the Al3+ concentration? 3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq)Answer: M
When the Hg²+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.737V. What is the Zn2+ concentration? Hg²"(aq) + Zn(s)→ Hg(1) + Zn²*(aq) Answer: M
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 7.66x10-³ atm, the H+ concentration is 1.18M, and the Co²+ concentration is 2.82×10-4M ? 2H+ (aq) + Co(s)→→→ H₂(g) + Co²+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: true

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When the Hg2+ concentration is 2.22×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.486V. What is the Cr³+ concentration? 3Hg²*(aq) + 2Cr(s)3Hg(1) + 2C1³*(aq) Answer: M

When the Hg2+ concentration is 2.22×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.486V. What is the Cr³+ concentration? 3Hg²(aq) + 2Cr(s)3Hg(1) + 2C1³(aq) Answer: M