When the Cu²+ concentration is 3.77x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.996V. What is the Zn²+ concentration?Cu²+ (aq) + Zn(s)→→→ Cu(s) + Zn²+ (aq)Answer:M When the Cu²+ concentration is 1.07 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.801 V. What is the Mg²+ concentration?Cu²+ (aq) + Mg(s) → Cu(s) + Mg2+ (aq)→ Cu(s) E = 0.337 Vred→ Mg(s) Fre = -2.370 VCu²+ (aq) + 2eMg²+ (aq) + 2e[Mg²+] =M

To determine the concentration of product, we will follow the following steps: 1) determine E°cell…

When the Cu²+ concentration is 1.07 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.801 V. What is the Mg2+ concentration? Cu²+ (aq) + Mg(s) → Cu(s) + Mg²+ (aq) red Cu²+ (aq) + 2e → Cu(s) Ed=0.337 V → Mg(s) E =-2.370 V Mg2+ (aq) + 2e red [Mg2+] = = M

When the Cu²+ concentration is 1.07 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.801 V. What is the Mg2+ concentration? Cu²+ (aq) + Mg(s) → Cu(s) + Mg²+ (aq) red Cu²+ (aq) + 2e → Cu(s) Ed=0.337 V → Mg(s) E =-2.370 V Mg2+ (aq) + 2e red [Mg2+] = = 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

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

Similar questions

When the Cu²+ concentration is 1.13 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.801 V. What is the Mg²+ concentration? Cu²+ (aq) + Mg(s) → Cu(s) + Mg²+ (aq) Cu²+ (aq) + 2e → Cu(s) Ed=0.337 V Mg2+ (aq) + 2e →Mg(s) E = -2.370 V red [Mg²+] - = M
What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions? PbO2(s) + 3 H+(aq) + HSO4−(aq) + 2 e− ↔ PbSO4(s) + 2 H2O(l) E0 = 1.690 V PbSO4(s) + H+(aq) + 2 e− ↔ Pb(s) + HSO4−(aq) E0 = −0.356 V
Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e – X(s) E° = -2.15 V Y3+ + 3 e –→ Y(s) E° = -0.29 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? E° 'cell V
8
A galvanic cell has the overall reaction: 2Cu+(aq) + Pb(s) → 2Cu(s) + Pb2+(aq) Which is the half reaction occurring at the cathode? Select one: Cu(s) → Cu+(aq) + e− Pb2+(aq) + e− → Pb+(aq) Pb(s) → Pb2+(aq) + 2e− Pb2+(aq) + 2e− → Pb(s) Pb(s) + 2e− → Pb2+(aq) Cu(s) + e− → Cu+(aq) Cu+(aq) + e− → Cu(s)
A galvanic cell is based on the following half-reactions (both written as reductions) at 25 °C: E° = 1.00 V VO₂+ (aq) + 2 H+ (aq) + e¯ ⇒ VO²+ (aq) + H₂O (1) Zn²+ (aq) + 2e → Zn (s) E° = -0.763 V Determine whether E is larger or smaller than Eº for the following case: [VO₂+] = 0.10 M, [H†] = 2.0 × 10˚² M, [VO²+] = 1.5 M, [Zn²+] = 0.45 M What is the change in Gibbs free energy for this reaction at standard state conditions (A,Gº)?
In the following: Al³+ (aq) + 3e → Al(s) E° = -1.66 V Cr³+ (aq) + 3e → Cr(s) E° = -0.74 V What is the standard cell potential for the corresponding galvanic cell? 0.00 V O-0.92 V +2.40 V +0.92 V O-2.40 V
what is the balanced chemical reaction for the galvanic cell that contains the two half reactions. Fe3+(aq) + 3e- → Fe(s) Eo=-0.036 V Mg2+(aq) + 2e-→ Mg(s) Eo=-2.37 V what is the state of matters?
When the Cu²+ concentration is 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.616 V. What is the Mn2+ concentration? Cu²+ (aq) + Mn(s) → Cu(s) + Mn²+ (aq) Cu2+ (aq) + 2e → Cu(s) Ed=0.337 V Mn²+ (aq) +2e → Mn(s) Fred =-1.180 V red [Mn²+] - M
Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions. An electrochemical cell is constructed based on the following balanced equation: Cu(s) + 2 Ag*(aq) → Cu2+(aq) + 2 Ag(s) Half-reactions with standard reduction potentials are given below. Cu2+(aq) + 2 e¯ → Cu(s); E° = 0.342 V Ag*(aq) + e¯ → Ag(s); E° = 0.800 V 5th attempt See Periodic Table O Se Calculate Ecell at 298 Kfor an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56 × 10 Mand [Cu2+] = 8.25 x 10-4 M. 3 V
When the Ag+ concentration is 1.44 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 3.269 V. What is the Mg2+ concentration? 2Ag+ (aq) + Mg(s) → 2Ag(s) + Mg²+ (aq) red Ag+ (aq) + e¯ → Ag(s) Eº = 0.799 V Mg²+ (aq) + 2e¯ → Mg(s) Fre = -2.370 V Mg²+] = M
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)