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Value of K for the given reaction has been
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08 Question (1 point) e See page 789 Calculate the value of K at 25°C for...
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...
please answer all of the questions!! 1. Which substance is reduced in the following reaction (1...
please answer all of the questions!!
1. Which substance is reduced in the following reaction (1 point): 2Al(s) + 3C12(g) → 2AlCl3(s) a. Al b. Cl2 c. AICI: d. None 2. Which substance is the reducing agent in the following reaction (1 point): 8H+ (aq) + MnO4 (aq) + 5Fe2+ (aq) → 5Fe3+ (aq) + Mn2+ (aq) + 4H2O(1) a. Fe2+ b. Mn04 c. H+ d. H20 3. Which substance is oxidized in the following reaction (1 point): Fes(s) +...
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,...
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...
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...
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...
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 +...
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)...
this is all we were given in class Calculate the value of AG for the following...
this is all we were given in class
Calculate the value of AG for the following reaction if [H2O2]i = [Fe] =1.0 M [OH']; = 1.3 x10-M, and [Fe3+] = 0.50 M. In which direction will this reaction have to shift in order to reach equilibrium? Explain your answer. Fe2(aq) + H2O2(aq) 5 Fe3+ (aq) + OH(aq) Standard-State Reduction Potentials and Half Rache Best reducing agents K + eK Bat +2 Ba Ca" + 2e Ca Na + c N...
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...
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...
please answer all of the questions!!
1. Which substance is reduced in the following reaction (1 point): 2Al(s) + 3C12(g) → 2AlCl3(s) a. Al b. Cl2 c. AICI: d. None 2. Which substance is the reducing agent in the following reaction (1 point): 8H+ (aq) + MnO4 (aq) + 5Fe2+ (aq) → 5Fe3+ (aq) + Mn2+ (aq) + 4H2O(1) a. Fe2+ b. Mn04 c. H+ d. H20 3. Which substance is oxidized in the following reaction (1 point): Fes(s) +...
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,...
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...
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...
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...
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 +...
this is all we were given in class
Calculate the value of AG for the following reaction if [H2O2]i = [Fe] =1.0 M [OH']; = 1.3 x10-M, and [Fe3+] = 0.50 M. In which direction will this reaction have to shift in order to reach equilibrium? Explain your answer. Fe2(aq) + H2O2(aq) 5 Fe3+ (aq) + OH(aq) Standard-State Reduction Potentials and Half Rache Best reducing agents K + eK Bat +2 Ba Ca" + 2e Ca Na + c N...
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