Determine what happens to the cell voltage when each of the following changes is made to the Daniell cell originally in standard conditions. Show the balanced equation for each reaction.

a) 2.25 M Zn(NO₃)₂ is added to the anode compartment
b) 2.25 M CuSO₄ is added to the cathode compartment
c) 1.00 M Cu(NO₃)₂ is added to the cathode compartment
d) 2.25 M H₂SO₄ is added to the cathode compartment

• A. a) E_cell is increased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  b) E_cell is increased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  c) Nothing happens to the cell voltage.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  d) E_cell is increased.
  Zn (s) + 2 H⁺ (aq) → Zn²⁺ (aq) + H₂ (g)
• B. a) E_cell is decreased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  b) E_cell is increased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  c) Nothing happens to the cell voltage.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  d) E_cell is decreased.
  Zn (s) + 2 H⁺ (aq) → Zn²⁺ (aq) + H₂ (g)
• C. a) E_cell is increased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  b) E_cell is decreased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  c) Nothing happens to the cell voltage.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  d) E_cell is increased.
  Zn (s) + 2 H⁺ (aq) → Zn²⁺ (aq) + H₂ (g)
• D. a) E_cell is decreased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  b) E_cell is increased.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  c) Nothing happens to the cell voltage.
  Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)
  
  d) E_cell is increased.
  Zn (s) + 2 H⁺ (aq) → Zn²⁺ (aq) + H₂ (g)

Answer: (B)