Use the standard reduction potentials given below to predict if a reaction will occur when Sn metal is put into a 1 M aqueous Cu²+ solution. Cu²+ (aq) + 2e¯ → Cu(s) Eº red Sn²+ (aq) + 2e¯ → Sn(s) Fº -0.140 V red - = 0.337 V If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. Submit Answer = (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + Retry Entire Group 9 more group attempts remaining

Use the standard reduction potentials given below to predict if a reaction will occur when Sn metal is put into a 1 M aqueous Cu²+ solution. Cu²+ (aq) + 2e¯ → Cu(s) Eº red Sn²+ (aq) + 2e¯ → Sn(s) Fº -0.140 V red - = 0.337 V If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. Submit Answer = (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + Retry Entire Group 9 more group 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...

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Use the standard reduction potentials given below to predict if a reaction will occur when Zn metal is put into a 1 M aqueous Ag solution. Ag+ (aq) + e → Ag(s) E red Zn²+ (aq) + 2e¯ → Zn(s) Ee -0.763 V Fred = 0.799 V 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.) + -> +
Use the standard reduction potentials given below to predict if a reaction will occur when Al metal is put into a 1 M Fe²+ solution. aqueous Fe2+ (aq) + 2e → Fe(s) E red Al³+ (aq) + 3e →→ Al(s) E + red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. ― -0.440 V -1.660 V (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X
Use 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.) +
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 1017
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG^0 for the following redox reaction. 2Br-(aq) + 2H2O(l) -> Br2(l) + H2(g) + 2OH−(aq) Be sure your answer has the correct number of significant digitss
Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. 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.) +
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.
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V red = Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be | than zero.
Calculate the cell potential given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.64 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.44 V
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.