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A Question Completion Status: 8 10 2+ +1.51 V Exhibit 17-1 Use this list of half-reactions...
55 61 7 8 9 10 +1.51 V +1 33 V Exhibit 17-1 Use this list...
55 61 7 8 9 10 +1.51 V +1 33 V Exhibit 17-1 Use this list of half-reactions to answer the following question(s). MnO4 (aq) + 8H+(aq) + 5e → Mn2+(aq) + 4H2O(1) Cr20,2(aq) + 6e → 2C++(aq) + 7H2O(1) Cu?+ (aq) + 2e → Cu(s) Pb2+ (aq) + 2e → Pb(s) Fe2+ (aq) + 2e → Fe(s) A13+ (aq) + 3e → Al(s) +0.34 V -0.13 V -0.44 V -1.66 V Refer to Exhibit 17-1. Which of these combinations...
Question Completion Status: 7 10 +1.517 -1.33 V Exhibit 17-1 Use this list of half-reactions to...
Question Completion Status: 7 10 +1.517 -1.33 V Exhibit 17-1 Use this list of half-reactions to answer the following question(s) MnO4 (aq) + 8H(aq) +5e → Mn++ (aq) + 4H2O(1) C12022-(aq) + 6e → 2013+(aq) + 7H2O(1) Cu2+ (aq) + 2e → Cu(s) Pb2+(aq) + 2e → Pb(s) Fe2+ (aq) + 2e → Fe(s) A1+ (aq) + 3e + Al(s) +0.34 V -0.13 v -0.44 V -1.66 V Refer to Exhibit 17-1. Determine Eºcell for the electrochemical cell designated by...
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...
how is cell potential become 1.51 - 1.19?? for question b. it was originally 1.51 /...
how is cell potential become 1.51 - 1.19?? for
question b.
it was originally 1.51 / 1.19 both positive.
then reversed second reaction (anode)
shouldn't it be 1.51 - (-1.19) so 2.7..?
8.3 Standard Reduction Po Also, since the two half-reactions invo anust be multiplied by integers as foilows lve different numhers of electrons 3(Mg--> Mg2+ + 2e-) %" (cathode)--1.66 V 2.37 V 2A13+ (aq) + 3Mg(s)-→ 2Al(s) + 3Mgat (aq) go (anode) l(cathode) (anode -1.66 V + 2.37 V...
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...
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...
Sodium metal is prepared by electrolysis of sodium chloride to the metal and chlorine gas. Using the...
Sodium metal is prepared by electrolysis of sodium
chloride to the metal and chlorine gas. Using the
reduction potentials attached, calculate E° and ΔG° for the overall
reaction.
TABLE 12.2 Standard Reduction Potentials at 25°C Half-reaction Eº, V Increasing strength as oxidizing agent Lit(aq) + e Li(s) K+(aq) + e → KS) Ba2+ (aq) + 2e → Ba(s) Sr2+(aq) + 2e → Sr(s) Ca2+(aq) + 2e → Ca(s) Na*(aq) + e Na(s) Mg2+ (aq) + 2e → Mg(s) Be2+(aq) + 2e...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
Use the information, below, to answer the next two (2) questions. Half-reaction (V) Cl2 + 2e + 2 C1° 1.36 Ag+ + e - Ag...
Use the information, below, to answer the next two (2) questions. Half-reaction (V) Cl2 + 2e + 2 C1° 1.36 Ag+ + e - Ag 0.80 Fe3+ + e + Fe2+ 0.77 Cu2+ + 2e - Cu 0.34 Ni2+ + 2e → Ni -0.25 A13+ + 3e + Al -1.66 (1) Which of the following species will oxidize Ni but not Ag? Cl2 O A13+ O Cu2+ O Cu Fe2+ Submit Answer Tries 0/2 (ii) Which of the following is...
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)...
55 61 7 8 9 10 +1.51 V +1 33 V Exhibit 17-1 Use this list of half-reactions to answer the following question(s). MnO4 (aq) + 8H+(aq) + 5e → Mn2+(aq) + 4H2O(1) Cr20,2(aq) + 6e → 2C++(aq) + 7H2O(1) Cu?+ (aq) + 2e → Cu(s) Pb2+ (aq) + 2e → Pb(s) Fe2+ (aq) + 2e → Fe(s) A13+ (aq) + 3e → Al(s) +0.34 V -0.13 V -0.44 V -1.66 V Refer to Exhibit 17-1. Which of these combinations...
Question Completion Status: 7 10 +1.517 -1.33 V Exhibit 17-1 Use this list of half-reactions to answer the following question(s) MnO4 (aq) + 8H(aq) +5e → Mn++ (aq) + 4H2O(1) C12022-(aq) + 6e → 2013+(aq) + 7H2O(1) Cu2+ (aq) + 2e → Cu(s) Pb2+(aq) + 2e → Pb(s) Fe2+ (aq) + 2e → Fe(s) A1+ (aq) + 3e + Al(s) +0.34 V -0.13 v -0.44 V -1.66 V Refer to Exhibit 17-1. Determine Eºcell for the electrochemical cell designated by...
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...
how is cell potential become 1.51 - 1.19?? for
question b.
it was originally 1.51 / 1.19 both positive.
then reversed second reaction (anode)
shouldn't it be 1.51 - (-1.19) so 2.7..?
8.3 Standard Reduction Po Also, since the two half-reactions invo anust be multiplied by integers as foilows lve different numhers of electrons 3(Mg--> Mg2+ + 2e-) %" (cathode)--1.66 V 2.37 V 2A13+ (aq) + 3Mg(s)-→ 2Al(s) + 3Mgat (aq) go (anode) l(cathode) (anode -1.66 V + 2.37 V...
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...
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...
Sodium metal is prepared by electrolysis of sodium
chloride to the metal and chlorine gas. Using the
reduction potentials attached, calculate E° and ΔG° for the overall
reaction.
TABLE 12.2 Standard Reduction Potentials at 25°C Half-reaction Eº, V Increasing strength as oxidizing agent Lit(aq) + e Li(s) K+(aq) + e → KS) Ba2+ (aq) + 2e → Ba(s) Sr2+(aq) + 2e → Sr(s) Ca2+(aq) + 2e → Ca(s) Na*(aq) + e Na(s) Mg2+ (aq) + 2e → Mg(s) Be2+(aq) + 2e...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
Use the information, below, to answer the next two (2) questions. Half-reaction (V) Cl2 + 2e + 2 C1° 1.36 Ag+ + e - Ag 0.80 Fe3+ + e + Fe2+ 0.77 Cu2+ + 2e - Cu 0.34 Ni2+ + 2e → Ni -0.25 A13+ + 3e + Al -1.66 (1) Which of the following species will oxidize Ni but not Ag? Cl2 O A13+ O Cu2+ O Cu Fe2+ Submit Answer Tries 0/2 (ii) Which of the following is...
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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