What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?
| Half-Reaction | E°(V) |
|---|---|
| Fe^(2+)(aq)+2e^(-)rarrFe(s) | -0.44 |
| Hg^(2+)(aq)+2e^(-)rarrHg(l) | 0.86 |
| Ag^(+)(aq)+e^(-)rarrAg(s) | 0.80 |
| Cu^(2+)(aq)+2e^(-)rarrCu(s) | 0.34 |
| Zn^(2+)(aq)+2e^(-)rarrZn(s) | -0.76 |
What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?
Hg²⁺(a q)+Fe(s) ⟶ Hg(l)+Fe²⁺(a q)
a) -40.5 kJ
b) -81.1 kJ
c) -125 kJ
d) -251 kJ
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What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s)...
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
Please combine the Mn electrode half reaction with the Ag electrode half reaction and write the...
Please combine the Mn electrode half reaction with the Ag
electrode half reaction and write the complete redox reaction using
date from table 8.1. Indicate which is the oxidizing and which is
the reducing agent.
b. Calculate the EMF when the reaction quotient (Q) =
]Mn2+]/[Ag+]^2 = 10^-5
Reducing agent Half-reaction E0 (volts) -2.93 2.87 Ca Na Mg Mn Zn Fe Ni Pb Ca Ca2++2e Na → Na++e- -2.36 Mn Mn++2e Zn Zn2++2e Fe → Fe2++ 2e- NiNi2++2e- -0.76 -0.47...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions you observed in a table as shown below. Write NR for “no reaction” where none was observed. 2+ (**e.g., Cu + Zn → Cu + Zn , Ecell = 1.10 V) Cu(NO3)2 Pb(NO3)2 Zn(NO3)2 16 Cu(s) NR NR Pb(s) NR Zn(s) NR 2. Calculate the Eº for every cell, whether or not a reaction was observed, using equation (5) and values for the standard...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶...
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Zn2+ + 2e- Zn(s) Eo = -0.76 V Cu+ + e- Cu(s) Eo = 0.52 A) -1.28 V B) +1.28 V C) 0.24 V D) -0.24 V E) +2.56 V 2.) For the redox reaction below, what is the Ecell if [Zn2+] = 0.072 M and [Cu+] = 1.27 M? T = 298 K Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Half Reactions:...
Given the E° table values on page 2, list and explain the following: 2. Which metals...
Given the E° table values on page 2, list and explain the following: 2. Which metals are capable of reducing Fe2 to Fe? Which metal ions are capable of oxidizing Zn to Zn2? E(volts) Half-Reaction +0.80 2 Ag ()+2 e2 Ag () Cura)+2 e Cu ( +0.34 +2e H2 0.0 2H (aq) Ni +2 e Ni ( -0.25 Fe()+2 e -0.44 Fe ( -0.76 Zn (a)+ 2 e Zn () Mg +2 e Mg ( -2.37 (aq) 2 K (a)+2...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
Find the best combination of half-cell pair from the following list, which will give the highest...
Find the best combination of half-cell pair from the following list, which will give the highest voltage. What is the voltage for that Galvanic cell? Given that Reduction Half-reaction Standard Potential (Eredo) Zn2+(aq) + 2e– → Zn(s) -0.763 (V) Fe2+(aq) + 2e– → Fe(s) -0.44 (V) Cu2+(aq) + 2e– → Cu(s) +0.34 (V) Sn2+(aq) + 2e– → Sn(s) -0.14 (V) Cu2+(aq) + e– → Cu+(aq) + 0.153 (V) Ag+(aq) + e– → Ag(s) + 0.80 (V) Cu+(aq) + e– →...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction Zn2 ag)2eZn Fe (a)2e Fe (s) Standard Reduction Potential at 25 °C, Volts 0.76 13 34 Cu2+ (aq) +2e- Cu (s) → Use the table above to predict voltlages for the redox couples studied in Part L, sections A and B. Redox Couple predicted voltage observed voltage 1. Zn/Cu 2. Zn/Pb 3. Pb/Cu 4. Fe/Cu 87 405
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
Please combine the Mn electrode half reaction with the Ag
electrode half reaction and write the complete redox reaction using
date from table 8.1. Indicate which is the oxidizing and which is
the reducing agent.
b. Calculate the EMF when the reaction quotient (Q) =
]Mn2+]/[Ag+]^2 = 10^-5
Reducing agent Half-reaction E0 (volts) -2.93 2.87 Ca Na Mg Mn Zn Fe Ni Pb Ca Ca2++2e Na → Na++e- -2.36 Mn Mn++2e Zn Zn2++2e Fe → Fe2++ 2e- NiNi2++2e- -0.76 -0.47...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions you observed in a table as shown below. Write NR for “no reaction” where none was observed. 2+ (**e.g., Cu + Zn → Cu + Zn , Ecell = 1.10 V) Cu(NO3)2 Pb(NO3)2 Zn(NO3)2 16 Cu(s) NR NR Pb(s) NR Zn(s) NR 2. Calculate the Eº for every cell, whether or not a reaction was observed, using equation (5) and values for the standard...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
Given the E° table values on page 2, list and explain the following: 2. Which metals are capable of reducing Fe2 to Fe? Which metal ions are capable of oxidizing Zn to Zn2? E(volts) Half-Reaction +0.80 2 Ag ()+2 e2 Ag () Cura)+2 e Cu ( +0.34 +2e H2 0.0 2H (aq) Ni +2 e Ni ( -0.25 Fe()+2 e -0.44 Fe ( -0.76 Zn (a)+ 2 e Zn () Mg +2 e Mg ( -2.37 (aq) 2 K (a)+2...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction Zn2 ag)2eZn Fe (a)2e Fe (s) Standard Reduction Potential at 25 °C, Volts 0.76 13 34 Cu2+ (aq) +2e- Cu (s) → Use the table above to predict voltlages for the redox couples studied in Part L, sections A and B. Redox Couple predicted voltage observed voltage 1. Zn/Cu 2. Zn/Pb 3. Pb/Cu 4. Fe/Cu 87 405
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
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