When the Hg2+ concentration is 1.63×104 M, the observedcell potential at 298K for an electrochemical cell with thefollowing reaction is 2.401V. What is the A13+ concentration?3Hg²+(aq) + 2Al(s)—>3Hg(1) + 2A13+(aq)Answer:M When the Hg2+ concentration is 8.18×104 M, the observedcell potential at 298K for an electrochemical cell with thefollowing reaction is 1.503V. What is the Cr3+ concentration?3Hg²+(aq) + 2Cr(s)—>3Hg(1) + 2Cr3+(aq)Answer: 1.49x10^ | M

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

Answered: When the Hg2+ concentration is 1.63×104…

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 Hg+ concentration is 1.44 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.717 V. What is the Zn2+ concentration? Hg (aq) + Zn(s) → Hg(1) + Zn²+ (aq) Zn M
Payal
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
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag* concentration is 6.38×10 4 M and the Zn2* concentration is 1.17 M ? 2+ 2Ag*(aq) + Zn(s)- →2Ag(s) + Zn²*(aq) Answer: V The cell reaction as written above spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.46 atm, the F" concentration is 6.08×10-3M, and the Pb2+ concentration is 5.78×10-4M ? F2(g) + Pb(s)- →2F*(aq) + Pb²+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Based on the cell potentials in the previous question calculate equilibrium constant of the following reaction H2(g) + I2 (g) → 2HI(aq) Please enter your answer using E notation with 2 decimals. for example, 1234.456 is written as 1.23E3
When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.279V. What is the Mg?+ concentration? 2Ag*(aq) + Mg(s)- →2Ag(s) + Mg²*(aq) Answer: M
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 1.69x10-4 M and the Mg2+ concentration is 1.43 M ? Pb2+ (aq) + Mg(s)→→→→ Pb(s) + Mg²+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: true false
When the Hg*+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.143V. What is the MIN2+ concentration? Hg* (aq) + Mn(s)→ Hg(1) + Mn²"(aq) Answer: M

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