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Imagine that the hypothetical elements. A B C and D form the ions A2+, B2, C2,...
Imagine that the hypothetical elements. A B C and D form the ions A2+, B2, C2, and Dar. The following reactions show the interactions that do or do NOT occur. Use this information to order the species in a reduction half reaction table. D2+ + C → C2+ + D Easiest to Hardest to Reduce Oxidize D2+ + B - No reaction C2+ + A - A2+ + C Hardest to Reduce Easiest to Oxidize st Lab Questions: To receive...
1. Predict if the following reactions will occur. If the reaction will occur, write out the...
1. Predict if the following reactions will occur. If the reaction will occur, write out the products. If a reaction will not occur, write "NR” for no reaction. Reactants Result Justification Ce3+(aq) + Cl2(g) NR Ce3+(aq) is higher than Cl2(g) Sn(s) + Ni2+(aq) Ag+(aq) + Au(s) Au3+(aq) + Ag(s) ce Li(s) + Ce4+(aq)
2. Indicate True or False for the following scenarios and explain if the reaction occurs using...
2. Indicate True or False for the following scenarios and explain if the reaction occurs using “higher than" and "lower than" using the sample table 3. True/False Scenario Justification Silver metal will dissolve in nitric acid, liberating H2 gas. Chromium metal can dissolve in dilute HCI. Oxygen in moist air can oxidize Fe2+ to Fe3+ Tin metal will reduce Co2+, but not Sn4+ 178 Page (intel V IA "ost Lab Questions: To receive full credit, you must SHOW ALL YOUR...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g)...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq)...
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq) 1.36 O2(g)+4H+(aq)+4e? ?2H2O(l) 1.23 Br2(l)+2e? ?2Br?(aq) 1.09 NO3?(aq)+4H+(aq)+3e? ?NO(g)+2H2O(l) 0.96 Ag+(aq)+e? ?Ag(s) 0.80 I2(s)+2e? ?2I?(aq) 0.54 Cu2+(aq)+2e? ?Cu(s) 0.16 2H+(aq)+2e? ?H2(g) 0 Cr3+(aq)+3e? ?Cr(s) -0.73 2H2O(l)+2e? ?H2(g)+2OH?(aq) -0.83 Mn2+(aq)+2e? ?Mn(s) -1.18 How can the table be used to predict whether or not a metal will dissolve in HCl? In HNO3? Drag the terms on the left to the appropriate blanks on the right to...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Zn + 2 Cr3+ + 2 Cr + 3 Zn? (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°? TABLE 18.1 Standard Reduction Potentials at 25°C EV) 2.87 1.61 1.51 1.36...
- cellpotentials and standard reduction potential table. -Determining the Nernst equation and finding the Faraday constant....
- cellpotentials and standard reduction potential table.
-Determining the Nernst equation and finding the Faraday
constant.
If you can explain how to solve for each part please.
25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e−...
Please show all steps taken (prefer typed solution)
Half-Reaction
E
°
(V)
Ag+ (aq) + e− → Ag (s)
0.7996
Al3+ (aq) + 3e− → Al (s)
−1.676
Au+ (aq) + e− → Au (s)
1.692
Au3+ (aq) + 3e− → Au (s)
1.498
Ba2+ (aq) + 2e− → Ba (s)
−2.912
Br2 (l) + 2e− → 2Br− (aq)
1.066
Ca2+ (aq) + 2e− → Ca (s)
−2.868
Cl2 (g) + 2e− → 2Cl− (aq)
1.35827
Co2+ (aq) + 2e−...
Imagine that the hypothetical elements. A B C and D form the ions A2+, B2, C2, and Dar. The following reactions show the interactions that do or do NOT occur. Use this information to order the species in a reduction half reaction table. D2+ + C → C2+ + D Easiest to Hardest to Reduce Oxidize D2+ + B - No reaction C2+ + A - A2+ + C Hardest to Reduce Easiest to Oxidize st Lab Questions: To receive...
1. Predict if the following reactions will occur. If the reaction will occur, write out the products. If a reaction will not occur, write "NR” for no reaction. Reactants Result Justification Ce3+(aq) + Cl2(g) NR Ce3+(aq) is higher than Cl2(g) Sn(s) + Ni2+(aq) Ag+(aq) + Au(s) Au3+(aq) + Ag(s) ce Li(s) + Ce4+(aq)
2. Indicate True or False for the following scenarios and explain if the reaction occurs using “higher than" and "lower than" using the sample table 3. True/False Scenario Justification Silver metal will dissolve in nitric acid, liberating H2 gas. Chromium metal can dissolve in dilute HCI. Oxygen in moist air can oxidize Fe2+ to Fe3+ Tin metal will reduce Co2+, but not Sn4+ 178 Page (intel V IA "ost Lab Questions: To receive full credit, you must SHOW ALL YOUR...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Zn + 2 Cr3+ + 2 Cr + 3 Zn? (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°? TABLE 18.1 Standard Reduction Potentials at 25°C EV) 2.87 1.61 1.51 1.36...
- cellpotentials and standard reduction potential table.
-Determining the Nernst equation and finding the Faraday
constant.
If you can explain how to solve for each part please.
25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
Please show all steps taken (prefer typed solution)
Half-Reaction
E
°
(V)
Ag+ (aq) + e− → Ag (s)
0.7996
Al3+ (aq) + 3e− → Al (s)
−1.676
Au+ (aq) + e− → Au (s)
1.692
Au3+ (aq) + 3e− → Au (s)
1.498
Ba2+ (aq) + 2e− → Ba (s)
−2.912
Br2 (l) + 2e− → 2Br− (aq)
1.066
Ca2+ (aq) + 2e− → Ca (s)
−2.868
Cl2 (g) + 2e− → 2Cl− (aq)
1.35827
Co2+ (aq) + 2e−...
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