Given the following information Ag+(aq) + e- ↔ Ag(s) Eºred = 0.799 V Ag2CrO4(s) + 2e-...

Given the following information

Ag⁺(aq) + e^- ↔ Ag(s) Eº_red = 0.799 V

Ag₂CrO₄(s) + 2e^- ↔ 2Ag(s) + CrO₄^2-(aq) Eº_red = 0.450 V

Determine the equilibrium constant at 25 °C for the reaction below:

Ag₂CrO₄(s) ↔ 2Ag⁺(aq) + CrO₄^2-(aq)

1.
9 × 10^-18

2.
1.6 × 10^-12

3.
1.2 × 10^-6

4.
1.6 × 10¹⁵

5.
1.7 × 10³⁹

Examine the following half reactions and select the strongest oxidizing agent among the species listed.

Cr²⁺(aq) + 2e^- ↔ Cr(s) Eº_red = -0.913 V

Sr²⁺(aq) + 2e^- ↔ Sr(s) Eº_red = -2.89 V

Fe²⁺(aq) + 2e^- ↔ Fe(s) Eº_red = -0.447 V

Co²⁺(aq) + 2e^- ↔ Co(s) Eº_red = -0.28 V

1.
Cr²⁺(aq)

2.
Fe(s)

3.
Fe²⁺(aq)

4.
Sr²⁺(aq)

5.
Co²⁺(aq)

2 points

QUESTION 5

Which of the changes below will increase the voltage of the following cell?

Co | Co²⁺ (0.010M) || H⁺ (0.010 M) | H₂(0.50 atm) | Pt

	1.	Increase the pressure of H₂ from 0.50 atm to 1.0 atm
	2.	Increase the concentration of H⁺ from 0.010 to 0.050 M.
	3.	Increase the mass of Co electrode from 12 grams to 15 g.
	4.	Increase the concentration of Co²⁺ from 0.010 M to 0.40 M.

Expert Solution

queen_honey_blossom answered 3 years ago

Reduction Half Reaction E (V) Ag2MoO4(s) + 2e- ---> 2 Ag(s) + MoO42-(aq) 0.4573 V Ag+(aq)...

Reduction Half Reaction E (V) Ag2MoO4(s) + 2e- ---> 2 Ag(s) + MoO42-(aq) 0.4573 V Ag+(aq) + e- ---> Ag(s) 0.7996 V a.) Calculate the mass in grams of Ag2MoO4(s) that will dissolve in 2.0 L of water. b.) Calcilate the cell potential of: Ag(s) | Ag2MoO4(s) | MoO42-(aq) (0.010 M) || Ag+(aq) (0.010M) | Ag (s)

Given: Pb2+(aq)+2e–⇌Pb(s);E°=–0.13 Mg2+(aq)+2e–⇌Mg(s);E°=–2.38V Ag+(aq)+e–⇌Ag(s);E°=0.80V 2H+(aq)+2e–⇌ H2(g);E°=0.00V Under standard-state conditions, which of the following species is the...

Given: Pb2+(aq)+2e–⇌Pb(s);E°=–0.13 Mg2+(aq)+2e–⇌Mg(s);E°=–2.38V Ag+(aq)+e–⇌Ag(s);E°=0.80V 2H+(aq)+2e–⇌ H2(g);E°=0.00V Under standard-state conditions, which of the following species is the best oxidizing agent? a. H b.Mg2+ c. Ag+ d. Pb e. Ag

Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45...

Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45 Zn2+(aq)+2e−→Zn(s) −0.76 Al3+(aq)+3e−→Al(s) −1.66 Mg2+(aq)+2e−→Mg(s) −2.37 1) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) 2) Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 3.80×10−4. Express your answer to three significant figures and include the appropriate units.

Calculate the Kf of Ag(NH3)2 + from Ag+(aq) + e- ⇋ Ag(s) E0= 0.81 V Ag(NH3)2+(aq)...

Calculate the Kf of Ag(NH3)2 + from Ag+(aq) + e- ⇋ Ag(s) E0= 0.81 V Ag(NH3)2+(aq) + e- ⇋ Ag(s) + 2NH3(aq) E0= 0.37 V

Half-reaction E° (V) Hg2+(aq) + 2e- -----> Hg(l) 0.855V Ni2+(aq) + 2e- -----> Ni(s) -0.250V Zn2+(aq)...

Half-reaction E° (V) Hg2+(aq) + 2e- -----> Hg(l) 0.855V Ni2+(aq) + 2e- -----> Ni(s) -0.250V Zn2+(aq) + 2e- -----> Zn(s) -0.763V (1) The weakest oxidizing agent is: ___ enter formula (2) The strongest reducing agent is: ___ (3) The strongest oxidizing agent is:___ (4) The weakest reducing agent is: ___ (5) Will Zn(s) reduce Hg2+(aq) to Hg(l)? _____(yes)(no) (6) Which species can be oxidized by Ni2+(aq)? ___ If none, leave box blank.

Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e-...

Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e- Al(s) -1.660V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Al(s) reduce Br2(l) to Br-(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank.

a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V

13)) a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will F-(aq) reduce Zn2+(aq) to Zn(s)? (6) Which species can be reduced by H2(g)? If none, leave box blank. b)) Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +...

Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) +...

Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) + 2e- ---> Pb(s) + SO42- (aq) E= -.356V Determine the Ksp for PbSO4(s) at 25 degrees C

NO3-(aq)+4H+(aq)+3e->NO(g)+2H2O(l) E=0.96V ClO2(g)+e->ClO2-(aq) E=0.95V Cu2+(aq)+2e->Cu(s) E=0.34V 2H+(aq)+2e->H2(g) E=0.00V Pb2+(aq)+2e->Pb(s) E=-0.13V Fe2+(aq)+2e->Fe(s) E=-0.45V Use appropriate data to...

NO3-(aq)+4H+(aq)+3e->NO(g)+2H2O(l) E=0.96V ClO2(g)+e->ClO2-(aq) E=0.95V Cu2+(aq)+2e->Cu(s) E=0.34V 2H+(aq)+2e->H2(g) E=0.00V Pb2+(aq)+2e->Pb(s) E=-0.13V Fe2+(aq)+2e->Fe(s) E=-0.45V Use appropriate data to calculate E?cell for the reaction. 3Cu(s)+2NO3-(aq)+8H+(aq)->3Cu2+(aq)+2NO(g)+4H2O(l) Express your answer using two decimal places.

Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V. Use...

Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V. Use the Nernst equation to calculate the cell potential for the cell described with standard line notation below. Zn|Zn2+(0.5082 M)||Cu2+(0.2699 M)|Cu Units are not required. Report answer to three decimal places. Please explain all of your steps! Thanks!

Question