1 balance the following equation in acidic solution using

Question

1. Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.

C₂H₆O(l) + Cr₂O₇^2-(aq) → C₂H₄O(l) + Cr³⁺(aq)

a.1

b.7

c.5

d.6

2. Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of H⁺.

H₂CO(aq) + S(s) => H₂S(g) + CO₂(g)

a. 4

b. 6

c. 2

d. 0

e. 1

3. Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water. 

Cl₂(aq) + S₂O₃^2- (aq) → Cl^-(aq) + SO₄^2-(aq)

a.3

b.1

c.5

d.6

e.2

4.Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water. 

MnO₄^-(aq) + SO₂(g) → Mn²⁺(aq) + HSO₄^-(aq)

a.4

b.6

c.2

d.5

e.3

5. Determine E^o for the following reaction, using the given standard reduction potentials:

Cu²⁺(aq) + Zn(s) → Cu(s) + Zn²⁺(aq) 

E^o for Zn²⁺(aq) = -0.76 V; 

E^o for Cu²⁺(aq) = 0.34 V

(Do not put in units)

Answer = ?

6. Determine E^o for the following reaction, using the given standard reduction potentials:

Sn(s) + Zn²⁺(aq) → Sn²⁺(aq) + Zn(s) 

E^o for Zn²⁺(aq) = -0.76 V; 

E^o for Sn²⁺(aq) = -0.14 V

(Do not put in units)

Answer = ?

7. Determine E^o for the following reaction, using the given standard reduction potentials:

Cr(s) + Fe²⁺(aq) → Cr³⁺(aq) + Fe(s) 

E^o for Fe²⁺(aq) = -0.44 V

E^o for Cr³⁺(aq) = -0.74 V

Do not put in units.

Answer = ?

8.Consider the following half-reactions.Which of these is the strongest reducing agent listed here? 

Au⁺(aq) + e^- → Au(s) E^o = 1.69 V

N₂O(g) + 2 H⁺(aq) + 2 e^- → N₂(g) + H₂O(l) E^o = 1.77 V

Cr³⁺(aq) + 3 e^- → Cr(s) E^o = -0.74 V

a..Au⁺(aq)

b.Au(s)

c.N₂O(g)

d.N₂(g)

e.Cr³⁺(aq)

f.Cr(s)

9. Identify the oxidizing agent and the reducing agent in the reaction.

3Cu(s) + 8H⁺(aq) + 2NO₃^-(aq) → 3Cu²⁺(aq) + 2NO(g) + 4H₂O(l)

a.oxidizing agent: Cu ; reducing agent: NO₃^-

b.oxidizing agent: NO₃^- ; reducing agent: Cu

c.oxidizing agent: H⁺ ; reducing agent: Cu

d.oxidizing agent: NO₃^- ; reducing agent: H⁺

^10. Consider the reaction between sulfite and a nonmetal anion, X^2-, to form the nonmetal, X, and thiosulfate: 

2 X^2-(aq) + 2 SO₃^2- + 3 H₂O(l) → 2 X(s) + S₂O₃^2- (aq) + 6 OH^- for which E^o_cell = 0.65. Given that the E^o_red for sulfite is -0.57 V, calculate E^o_red for X. Enter your answer to 2 decimal places.