Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactionsHalf-reaction8° (V)Half-reactionF₂ +2e2F-Ag2+ + eAg+Co³+ + e→→ Co²+H₂O₂ + 2H+ + 2eCe4++e Ce³+→ 2H₂OPbO₂ + 4H+ + SO42MnO4 + 4H+ + 3eIO4 + 2H+ + 2e →MnO4 + 8H+ + SeAu³+ + 3e → AuPbO₂ + 4H+ + 2eCl₂ +2e2C1-Hg₂2+ + 2eFe³+ + e+2e →→ PbSO4 + 2H₂O→ MnO₂ + 2H₂OIO3 + H₂O→ Mn²+ + 4H₂O→ Pb²+ + 2H₂OCr₂O72- + 14H+ + 6e- →2Cr³+ + 7H₂OO₂ + 4H+ + 4e → 2H₂OMnO₂ + 4H+ + 2eIO3 + 6H+ + Se-Br₂ 2e 2BrVO₂+ + 2H+ + eAuCl4 + 3e →NO3 + 4H+ClO₂ + e2Hg2+ + 2eAge → Ag→ Mn²+ + 2H₂O→ 1₂ + 3H₂O→ VO2+ + H₂OAu + 4CI-+ 3e → NO + 2H₂OClO₂-→ Hg₂²+→ 2HgFe2+O₂ + 2H+ + 2e → H₂O₂MnO4 + e→→ MnO4²-1₂ +2e → 21-CuteCu2.871.991.821.781.701.691.681.601.511.501.461.361.331.231.211.201.091.000.990.960.9540.910.800.800.770.680.560.540.52O₂ + 2H₂O + 4e4OH-Cu2+ + 2e → CuHg₂Cl₂ + 2e →→ 2Hg + 2Cl-AgCl +eAg + Cl-SO4 + 4H+ + 2eCu²+ + e2H+ + 2eFe³+ + 3eCu+→→ H₂→→ Fe→→ Pb→→ Sn→→ NiPb²+ + 2eSn²+ + 2eNi2+ + 2ePbSO4 + 2eCd2+ + 2e→→ Pb + SO4²-→→ Cd→→→ FeFe2+ + 2eCr³+ + eCr²+Cr³+ + 3e→ Cr→ ZnZn²+ + 2e2H₂O + 2e→ H₂ + 2OH-Mn²+ + 2e → MnAl³+ + 3e →→ AlH₂ +2e → 2H-Mg2+ + 2e → MgLa³+ + 3e → La→→→ NaNa+ + eCa2+ + 2eBa2+ + 2eK++eK→→ Ca→→ Ba→ H₂SO3 + H₂OLite Li8° (V)0.400.340.270.220.200.160.00-0.036-0.13-0.14-0.23-0.35-0.40-0.44-0.50-0.73-0.76-0.83-1.18-1.66-2.23-2.37-2.37-2.71-2.76-2.90-2.92-3.05 Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, , or > symbolto separate substances in the list.)Al3+, Cr³+, Zn2+, H₂O, 104, and 1₂chemPad|XX"HelpGreek-

Use data from standard reduction potential table and place the following in order of increasing…

Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, =, or > symbol to separate substances in the list.) Al3+, Cr3+, Zn2+, H₂O, 104, and 1₂ chemPad XX→← Help Greek

Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, =, or > symbol to separate substances in the list.) Al3+, Cr3+, Zn2+, H₂O, 104, and 1₂ chemPad XX→← Help Greek

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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A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.08 V (minus 1.08 V).
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A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.09 V (minus 1.09 V).
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Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Cd2+ (aq) + Zn(s)→→→→→→ Cd(s) + Zn²+ (aq) Answer: kJ K for this reaction would be than one.
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