RedOx Reactions

Front

E⁰ values: Br/Br^- = + 1.90; Ag⁺/Ag(s)=0.80 Cu²⁺/Cu(s) = + 0.34; I² (s)/I^– =+0.54. Which species will Cu reduce?

Back

Cu will reduce Br₂

Front

Identify the oxidizing agent in the reaction: 4NH₃ + 3O₂ (g) → 2N₂ (g) + 6H₂O (g)

Back

O₂

Front

What is the reducing agent in the reaction? Fe₂O₃ (s) + 3CO (g) -----→ 2Fe (s) + 3CO₂ (g)

Back

CO

Front

Reduction half cell reaction for Fe²⁺ + H⁺ + Cr₂O₇^2– ----→ Cr³⁺ + Fe³⁺ + H₂O

Back

H⁺ + Cr₂O₇^2– ----→ Cr³⁺ + H₂O

Front

In which substance does sulfur have a negative oxidation number? Options: CaSO₄, S, SO₂, Na₂S

Back

Na₂S

Front

Calculate the standard cell emf for the following cell: Mg |Mg²⁺ || NO₃^- (acid soln)| NO(g) | Pt

Back

3.33V

Front

Which of the following species is the strongest oxidizing agent under standard-state conditions? Ag⁺(aq), H₂(g), H⁺(aq), Cl₂(g), Al³⁺(aq)

Back

Cl₂(g)

Front

For the reaction Ni²⁺(aq) + 2Fe²⁺(aq) → Ni(s) + 2Fe³⁺(aq), What is the standard cell potential E°_cell?

Back

-1.02V

Front

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

Back

E°_cell is always positive.

Front

For the electrochemical cell Ni(s) | Ni²⁺(1 M) || H⁺(1 M) | H₂(1 atm) | Pt(s), which change will cause a decrease in the cell voltage? Options: Increase the pressure of H₂ to 2.0 atm, Decrease the mass of the nickel electrode, Lower the pH of the cell electrolyte, Decrease the concentration of Ni²⁺ ion, none of these.

Back

Increase the pressure of H₂ to 2.0 atm.