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.

Expert Solution

queen_honey_blossom answered 1 year ago

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.

Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and...

Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and Sn4+(aq) + 2e− → Sn2+(aq) does not equal the potential for the reaction Sn4+(aq) + 4e−→ Sn(s). What is the net cell potential? Compare the values of ΔG° for the sum of the potentials and the actual net cell potential.

Decide whether or not each metal dissolves in 1 molL?1HCl(aq). Reduction Half-Reaction E?(V) Al3+(aq)+3e? ?Al(s) -1.66...

Decide whether or not each metal dissolves in 1 molL?1HCl(aq). Reduction Half-Reaction E?(V) Al3+(aq)+3e? ?Al(s) -1.66 Mg2+(aq)+2e? ?Mg(s) -2.37 Ag+(aq)+e? ?Ag(s) 0.80 Au3+(aq)+3e? ?Au(s) 1.50 Pb2+(aq)+2e? ?Pb(s) -0.13 Cd2+(aq)+2e? ?Cd(s) -0.40 a) Write a balanced redox reaction showing what happens when Al dissolves. Express your answer as a chemical equation. Identify all of the phases in your answer. b) Write a balanced redox reaction showing what happens when Pb dissolves. Express your answer as a chemical equation. Identify all of...

Decide whether or not each metal dissolves in 1 molL−1HCl(aq). Reduction Half-Reaction E∘(V) Al3+(aq)+3e− →Al(s) -1.66...

Decide whether or not each metal dissolves in 1 molL−1HCl(aq). Reduction Half-Reaction E∘(V) Al3+(aq)+3e− →Al(s) -1.66 Mg2+(aq)+2e− →Mg(s) -2.37 Ag+(aq)+e− →Ag(s) 0.80 Au3+(aq)+3e− →Au(s) 1.50 Pb2+(aq)+2e− →Pb(s) -0.13 Cd2+(aq)+2e− →Cd(s) -0.40 Will a) Al dissolves does not dissolve b) Ag dissolves does not dissolve c) Pb dissolves does not dissolve

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.

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)

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

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) +...

Consider the following reaction: Br2(l) + 2I-(aq) ---> 2Br-(aq) + I2(s) a.Calculate ΔGorxn b.Calculate K

The standard cell potential, E°, for Br2(aq) + Zn(s) → 2Br-(aq) + Zn2+(aq) at 298K is...

The standard cell potential, E°, for Br2(aq) + Zn(s) → 2Br-(aq) + Zn2+(aq) at 298K is 1.82V. Calculate the value of ΔG° in kJ. Use 96,485 C/mol e-. Then calculate the equilibrium constant for the data.

Question