TUTOR Calculate the Concentration of a Species Using Cell Voltage When [Hg2+] = 1.16 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 3 Mg2+ concentration in this cell? Hg2+(aq) + Mg(s) → Hg(t) + Mg²+(aq) [Mg2+] = 4.36x10^-6 x mol/L Resubmit Show Approach Show Tutor Steps Submit Answer Try Another Version 2 item attempts remaining

TUTOR Calculate the Concentration of a Species Using Cell Voltage When [Hg2+] = 1.16 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 3 Mg2+ concentration in this cell? Hg2+(aq) + Mg(s) → Hg(t) + Mg²+(aq) [Mg2+] = 4.36x10^-6 x mol/L Resubmit Show Approach Show Tutor Steps Submit Answer Try Another Version 2 item attempts remaining

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

please answer both When the Cu2+ concentration is 9.97x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.425V. What is the Mn2+ concentration? Cu2+ (aq) + Mn(s) Cu(s) + Mn²+ (aq) Answer: M 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) E=0.337 V Mn²+ (aq) + 2e → Mn(s) Fred red E-1.180 V [Mn²+] - M
Given the standard electrode reduction potentials, which reaction will occur spontaneously?
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.37×10-3 atm, the H* concentration is 1.04M, and the Mg2+ concentration is 7.01×10-4M ? 2H (аq) + Mg(s)—— Н2(g) + - Mg2*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations give v true false Submit Answer Retry Entire Group 9 more group attempts remaining
Help on these two please
Item 1 < 1 of 25 Constants | Periodic Table Part A The standard cell potential (E') of the reaction below is -0.55 V. The value of A G for the reaction is J/mol. I2 (5) + 2Br (aq) → 21 (aq) + Brz (1) O 1.1- 105 O 0.54 O 0.55 O 5.5 - 106 O none of the above Submit Request Answer
image #7
eq Preq 1req F2 # 3 LU E D What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 8.54 x 10-4 M and the Mg2+ concentration is 1.23 M ? Ecell F3 The cell reaction as written above is Submit Answer $ SA 4 2+ Pb²+ (aq) + Mg(s) → Pb(s) + Mg²+ (aq) R F V V F4 % References] Use the References to access important values if needed for this question. стор T Retry Entire Group G DII Cengage Learning Cengage Technical Support F5 OL Y H F6 9 more group attempts remaining & 7 U ✓for the concentrations given. F7 J OO PrtScn BN M F8 K Home F9 L End F10 Previous PgUp F11 Next Save and Exit 4x10 PgDn 8:28 PM 12/2/2022 F12 1 Ins {
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg2+ (0.17 M) || Mg2+ (0.85 M) | Mg(s) V
Q4 A: What is the E for the Fe3+/Fe2+ half-cell if [Fe3+] = 0.001 M and [Fe2+] is 0.1 M at 25 °C? if you know Fe reduction potential = + 0.771 V *
If an alkaline battery produces a cell potential of 1.50 V, what is the value of AGcell? The half-reactions in alkaline batteries are: ZnO(s) + H,0(1) + 2e¯ → Zn(s) + 20H¯(aq) 2MnO, (s) +H,0(1) +2e¯ Mn,0, (s) +20H (ag) 1st attempt l See Periodic Table AGcell = kJ
O ADVANCED MATERIAL Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential NO, (aq)+4H (aq)+3e¯ → NO(g)+2 H,O(1) E red = +0.96 V Cl,(9)+2e + 2 Cl (ag) = +1.359 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer ||V here. Round your answer to 2 significant digits.
10