Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:When the Cu?+ concentration is 1.31 M, the observed
cell potential at 298K for an electrochemical cell with
the following reaction is 2.808V. What is the Mg²+
concentration?
2+
Cu2"(aq) + Mg(s)→ Cu(s) + Mg“(aq)
Answer:
M
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- Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)arrow_forwardWhat is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 9.40 × 10-4 M and the Zn²+ concentration is 1.18 M? Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq) Pb2+ (aq) + 2e7 →→ Pb(s) E red Zn²+ (aq) + 2e → Zn(s) Ee red Ecell = -0.126 V = -0.763 V Otrue Ofalse = The cell reaction as written above is spontaneous for the concentrations given:arrow_forwardWhen 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 Marrow_forward
- When the Hg2+ concentration is 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the following 2+ reaction is 3.318 V. What is the Mg²+ concentration? 2+ Hg²+ (aq) + Mg(s) → Hg(1) + Mg²+ (aq) red Hg2+ (aq) + 2e → Hg(1) E 0.855 V → Mg(s) Fred Mg2+ (aq) + 2e = -2.370 V [Mg²+] = Submit Answer M Retry Entire Group = 7 more group attempts remainingarrow_forwardWhen the Ag concentration is 1.00 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.530 V. What is the A1³+ concentration? 3+ 3Ag+ (aq) + Al(s) → 3Ag(s) + Al³+ (aq) red Ag+ (aq) + e → Ag(s) Ed Al³+ (aq) + 3e → Al(s) Ee red [A1³+] = M 0.799 V = -1.660 Varrow_forwardWhat is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 1.14 x 10-4 M and the Mn²+ concentration is 1.05 M? 2Ag (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag (aq) +e → Ag(s) Fred=0.799 V Mn²+ (aq) + 2e → Mn(s) E= -1.180 V Ecell = V The cell reaction as written above is spontaneous for the concentrations given: O true O falsearrow_forward
- When the Ag+ concentration is 1.26 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.267V. What is the Mg2+ concentration? 2Ag+(aq) + Mg(s)2Ag(s) + Mg2+(aq)arrow_forwardWhen the Pb²+ concentration is 1.14 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.154 V. What is the Mn²+ concentration? 2+ Pb²+ (aq) + Mn(s) → Pb(s) + Mn²+ (aq) 2+ Pb²+ (aq) + 2e¯¯ → Pb(s) Fre (aq) + 2e¯ → Mn(s) E Mn²+ red 2+ Mn²+] = M -0.126 V -1.180 Varrow_forwardBhu Please don't provide the handwriting solutionarrow_forward
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