Use the redox table below to answer the following questions. a) Would MnO2 reduce Cu2+? b)...
Use the redox table below to answer the following questions.
a) Would MnO2 reduce Cu2+?
b) Would Mn2+ reduce Cu2+?
c) Would MnO2 oxidize Cu2+?
d) Would MnO2 oxidize Cu+?
e) Would MnO2 oxidize Cu0?
f) Would Cr3+ reduce Ni2+?
g) Would Cr2+ reduce Ni2+?
h) Would O2 oxidize Au ( at pH= 0)?
i) Would O2 oxidize Au in the presence of Cl– ions (at pH= 0)?
j) Would O2 oxidize Pb2+ ?
k) Would PbO2 oxidize H2O (at pH= 0)?
Homework Answers
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Use the redox table below to answer the following questions.
a) Would MnO2 reduce Cu2+?
b)...
For all of the following experiments, under standard conditions, which species could be spontaneously produced? A...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
1. How do I read the half reaction table? 2. If im asked for the best...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
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...
the first picture is about some useful information, and the second picture is the question that...
the first picture is about
some useful information, and the second picture is the question
that bothers me. I wonder how we know the half-cell reaction of it.
Please explain!!!
TABLE 18.1 | Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 Half-Reaction F2 + 2e →2F Ag2+ + e +Agt Co3- + e + CO2- H2O2 + 2H+ + 2e +2H20 Ce+ + e + Ce+ PbO2 +...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for use in their design are given in the table below. Assume the ambient Martian temperature is -67.5*C, 205.7 K. What electrode combination (assume 0.1 M solutions) would provide the 1.317 V required by the spacecraft electronics? Use Appendix 11 for your standard cell potentials. А Rh+ +e- Rh/Ni2+ + 2e + NI O B Rh+ + e + Rh/Cr3+ + 3e - Cr C...
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...
12. Considering the following electrochemical cell carried out at 25°C and using only the informa...
12. Considering the following electrochemical cell carried out at 25°C and using only the information in the table below: MnO2 (s) Cu (s)4 H (a) Mn2 (a) Cu2 (aq)2 H2O (0) Substance AH (kJ/mol) 0.00 219.4 0.00 285.8 64.9 520.0 AS (J/mol Cu (s) 33.2 78.8 0.00 70.0 98.0 53.1 H2O Cu (aq) MnO2 (s) a) If this system were at equilibrium, in what direction would the reaction go to re-attain its state of equilibrium if the temperature were incre...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq,...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
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...
the first picture is about
some useful information, and the second picture is the question
that bothers me. I wonder how we know the half-cell reaction of it.
Please explain!!!
TABLE 18.1 | Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 Half-Reaction F2 + 2e →2F Ag2+ + e +Agt Co3- + e + CO2- H2O2 + 2H+ + 2e +2H20 Ce+ + e + Ce+ PbO2 +...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for use in their design are given in the table below. Assume the ambient Martian temperature is -67.5*C, 205.7 K. What electrode combination (assume 0.1 M solutions) would provide the 1.317 V required by the spacecraft electronics? Use Appendix 11 for your standard cell potentials. А Rh+ +e- Rh/Ni2+ + 2e + NI O B Rh+ + e + Rh/Cr3+ + 3e - Cr C...
12. Considering the following electrochemical cell carried out at 25°C and using only the information in the table below: MnO2 (s) Cu (s)4 H (a) Mn2 (a) Cu2 (aq)2 H2O (0) Substance AH (kJ/mol) 0.00 219.4 0.00 285.8 64.9 520.0 AS (J/mol Cu (s) 33.2 78.8 0.00 70.0 98.0 53.1 H2O Cu (aq) MnO2 (s) a) If this system were at equilibrium, in what direction would the reaction go to re-attain its state of equilibrium if the temperature were incre...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
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