Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Consult a table of reduction potentials and determine which two metals are capable of reducing iron (II) to iron under standard conditions.
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Sn, Pb
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Al, Mg
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Mg, Cu
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Ca, Sn
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Cd, Hg
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- Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Mn metal is put into a 1M aqueous Al3+ solution.If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. + +arrow_forwardCalculate the standard cell potential, E, for the equation Cr(s) + F,(g) → Cr**(aq) + 2F (aq) Use the table of standard reduction potentials. E• cell %3D Varrow_forwardUse standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 31₂ (s) + 2Cr(s) → 61¯(s) + 2Cr³+ (aq) I₂ (s) + 2e¯ → 21¯ (s) Cr³+ r³+ (aq) + 3e¯ → Cr(s) E red kJ AGO = Eº = = 0.535 V red = -0.740 Varrow_forward
- Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Cd²+ (aq) + Zn(s) → Cd(s) + Zn²+ (aq) AG⁰ = Cd2+ (aq) +2e → Cd(s) E red Zn²+ (aq) +2e → Zn(s) E red K for this reaction would be greater less = -0.403 V -0.763 V kJ than one.arrow_forwardRank the following in increasing ability as oxidizing agents. The reduction potentials of all species are shown below. Cl, (g) + 2e → 2C1 (aq) E° = 1.3583 V Ag*(aq) + le Cu²+ (aq) + 2e¯ → Ag(s) E° = 0.7996 V → Cu(s) E° = 0.342 V Sn²+ (aq) + 2e → Sn(s) E° = - 0.136 V к"(ад) + 1е — → K(s) E° - 2.95 V 1st attemptarrow_forwardUse standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Co²+ (aq) + Zn(s) → Co(s) + Zn²+ (aq) red Co²+ (aq) + 2e → Co(s) Ee Zn²+ (aq) + 2e¯ → Zn(s) Ee red AGO K for this reaction would be kJ = -0.280 V -0.763 V than one.arrow_forward
- According to Standard reduction potentials table on page 164 (OLI), which of the following metals would reduce Sn (tin) from its solution? Sn+2 + 2e Sn O Au (gold) O Fe (Iron) O Pb (lead) O Cu (copper)arrow_forwardUse standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Pb²+ (aq) + Cu(s) - → Pb(s) + Cu²+ (aq) AG° Pb²+ (aq) + 2e¯¯ → Pb(s) Ee Cu²+ (aq) + 2e¯ → Cu(s) Fre red = kJ K for this reaction would be = -0.126 V = 0.337 V + than one.arrow_forwardUse the standard reduction potentials given below to predict if a reaction will occur when Mg metal is put into a 1 M aqueous Cd²+ solution. Cd(s) Eº = -0.403 V red Eº → Mg(s) Fred = -2.370 V Cd2+ (aq) + 2e → 2+ Mg²+ (aq) + 2e If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +arrow_forward
- Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017arrow_forwardUsing standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy Be sure your answer has the correct number of significant digits. 3+ 4Fe²+ (aq) + O₂(g) + 4H* (aq) → 4Fe³+ (aq) + 2H₂O (1) KJ x10 X Ś AGO for the following redox reaction.arrow_forwardStandard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?arrow_forward
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