hello, i need hlep with part a and b. last answers you provided were wrong . handwritten solutions are prefered. 1a) Assuming standard conditions, answer the following questions.(Use the table of Standard Reduction Potentials for common Half-reactions i attached belowIf hydrogen is one of the reagents, assume acidic solution.). write yes or no beside each one. Is Ag+(aq) capable of oxidizing H2(g)? Is Fe2+(aq) capable of reducing VO2+(aq)? Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)? Is Ni2+(aq) capable of oxidizing H2(g)? Is Fe2+(aq) capable of reducing Sn2+(aq) to Sn metal? Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)? 1b) Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, attached below, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6". Al Ca H2 (acidic half-cell solution) Fe Pb2+ (acidic half-cell solution) Fe2+ Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactionsHalf-reaction%° (V)Half-reactionF₂ +2e7 →2F-Ag²+ + e → Ag+Co³+ + e→→ Co²+H₂O₂ + 2H+ + 2e7 → 2H₂OCe4+ + e→Ce³+PbO₂ + 4H+ + SO4² +2e →→ PbSO4 + 2H₂OMnO4 + 4H+ + 3e7 → MnO₂ + 2H₂OIO4 + 2H+ + 2e → IO3 + H₂OMnO4 + 8H+ + 5e → Mn²+ + 4H₂OAu³+ + 3e7 → AuPbO₂ + 4H+ + 2e¯ → Pb²+ + 2H₂OCl₂ +2e2C1-Cr₂O2 + 14H+ + 6e¯ → 2Cr³+ + 7H₂OO₂ + 4H+ + 4e → 2H₂OMnO₂ + 4H+ + 2eIO3 + 6H+ + 5e-Br₂ +2e7 → 2Br→ Mn²+ + 2H₂O1₂+ 3H₂OVO₂+ + 2H+ + e → VO²+ + H₂OAuCl4 + 3e → Au + 4Cl-NO3 + 4H+ + 3e → NO + 2H₂OCIO₂ + e→→ CIO₂2Hg2+ + 2c7 → Hg₂²+Ag+ + e → AgHg₂+ + 2e →→ 2HgFe³+ + e Fe2+O₂ + 2H+ + 2e → H₂O₂MnO4 + e→→ MnO4²-21-1₂ +2eCut + e → Cu2.871.991.821.781.701.691.681.601.511.501.461.361.331.231.211.201.091.000.990.960.9540.910.800.800.770.680.560.540.52O₂ + 2H₂O + 4c→ 40HCu²+ + 2e →→ CuHg₂Cl₂ + 2e →→ 2Hg + 2Cl-AgCleAg + Cl-SO4²- + 4H+ + 2e¯ → H₂SO3 + H₂OCu²+ + e→ Cu+2H+ + 2e7 → H₂→→ Fe→→ Pb→ Sn→ NiFe³+ + 3ePb²+ + 2eSn²+ + 2e7Ni²+ + 2e7PbSO4 + 2eCr³+ + e→→Cd²+ + 2e7→ CdFe2+ + 2e7 → FeCr²+→ Cr→ ZnCr3+ + 3e-Zn²+ + 2e72H₂O + 2e→ H₂ + 2OH-Mn²+ + 2e7 → MnAl³+ + 3e → AlH₂ +2e7 → 2H-Mg2+ + 2c→→ MgLa³+ + 3e7 → LaNa+ + e- → NaCa²+ + 2e7 → CaBa2+ + 2e7 → BaK+ + e→→ KLite Li→→ Pb + SO4²-8° (V)0.400.340.270.220.200.160.00-0.036-0.13-0.14-0.23-0.35-0.40-0.44-0.50-0.73-0.76-0.83-1.18-1.66- 2.23-2.37-2.37-2.71-2.76-2.90-2.92-3.05

The species with the standard reduction potential greater than H+ would oxidize the H2.

Answered: 1a) Assuming standard conditions,…

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hello, i need hlep with part a and b. last answers you provided were wrong . handwritten solutions are prefered.

1a) Assuming standard conditions, answer the following questions.
(Use the table of Standard Reduction Potentials for common Half-reactions i attached below
If hydrogen is one of the reagents, assume acidic solution.). write yes or no beside each one.

    Is Ag⁺(aq) capable of oxidizing H₂(g)?
    Is Fe²⁺(aq) capable of reducing VO₂⁺(aq)?
    Is Sn metal capable of reducing Fe³⁺(aq) to Fe²⁺(aq)?
    Is Ni²⁺(aq) capable of oxidizing H₂(g)?
    Is Fe²⁺(aq) capable of reducing Sn²⁺(aq) to Sn metal?
    Is Cr³⁺(aq) capable of oxidizing Fe²⁺(aq) to Fe³⁺(aq)?

1b) Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, attached below, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6".

        Al
        Ca
        H₂ (acidic half-cell solution)
        Fe
        Pb²⁺ (acidic half-cell solution)
        Fe²⁺

Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions
Half-reaction
%° (V)
Half-reaction
F₂ +2e7 →2F-
Ag²+ + e → Ag+
Co³+ + e→→ Co²+
H₂O₂ + 2H+ + 2e7 → 2H₂O
Ce4+ + e→Ce³+
PbO₂ + 4H+ + SO4² +2e →→ PbSO4 + 2H₂O
MnO4 + 4H+ + 3e7 → MnO₂ + 2H₂O
IO4 + 2H+ + 2e → IO3 + H₂O
MnO4 + 8H+ + 5e → Mn²+ + 4H₂O
Au³+ + 3e7 → Au
PbO₂ + 4H+ + 2e¯ → Pb²+ + 2H₂O
Cl₂ +2e2C1-
Cr₂O2 + 14H+ + 6e¯ → 2Cr³+ + 7H₂O
O₂ + 4H+ + 4e → 2H₂O
MnO₂ + 4H+ + 2e
IO3 + 6H+ + 5e-
Br₂ +2e7 → 2Br
→ Mn²+ + 2H₂O
1₂+ 3H₂O
VO₂+ + 2H+ + e → VO²+ + H₂O
AuCl4 + 3e → Au + 4Cl-
NO3 + 4H+ + 3e → NO + 2H₂O
CIO₂ + e→→ CIO₂
2Hg2+ + 2c7 → Hg₂²+
Ag+ + e → Ag
Hg₂+ + 2e →→ 2Hg
Fe³+ + e Fe2+
O₂ + 2H+ + 2e → H₂O₂
MnO4 + e→→ MnO4²-
21-
1₂ +2e
Cut + e → Cu
2.87
1.99
1.82
1.78
1.70
1.69
1.68
1.60
1.51
1.50
1.46
1.36
1.33
1.23
1.21
1.20
1.09
1.00
0.99
0.96
0.954
0.91
0.80
0.80
0.77
0.68
0.56
0.54
0.52
O₂ + 2H₂O + 4c→ 40H
Cu²+ + 2e →→ Cu
Hg₂Cl₂ + 2e →→ 2Hg + 2Cl-
AgCleAg + Cl-
SO4²- + 4H+ + 2e¯ → H₂SO3 + H₂O
Cu²+ + e→ Cu+
2H+ + 2e7 → H₂
→→ Fe
→→ Pb
→ Sn
→ Ni
Fe³+ + 3e
Pb²+ + 2e
Sn²+ + 2e7
Ni²+ + 2e7
PbSO4 + 2e
Cr³+ + e→→
Cd²+ + 2e7
→ Cd
Fe2+ + 2e7 → Fe
Cr²+
→ Cr
→ Zn
Cr3+ + 3e-
Zn²+ + 2e7
2H₂O + 2e
→ H₂ + 2OH-
Mn²+ + 2e7 → Mn
Al³+ + 3e → Al
H₂ +2e7 → 2H-
Mg2+ + 2c→→ Mg
La³+ + 3e7 → La
Na+ + e- → Na
Ca²+ + 2e7 → Ca
Ba2+ + 2e7 → Ba
K+ + e→→ K
Lite Li
→→ Pb + SO4²-
8° (V)
0.40
0.34
0.27
0.22
0.20
0.16
0.00
-0.036
-0.13
-0.14
-0.23
-0.35
-0.40
-0.44
-0.50
-0.73
-0.76
-0.83
-1.18
-1.66
- 2.23
-2.37
-2.37
-2.71
-2.76
-2.90
-2.92
-3.05

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