Qstnid -Ii-5- Write The Nernst Equation And Emf Of The Following Cells At 298 K: () Mg(s) | Mg2+(0.001m) || Cu2+(0.0001 M) | Cu(s) () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Mg(s) | Mg2+(0.001m) || Cu2+(0.0001 M) | Cu(s) () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). () Fe(s) | Fe2+(0.001m) || H+(1m)|h2(g)(1bar) | Pt(s) () Sn(s) | Sn2+(0.050 M) || H+(0.020 M) | H2(g) (1 Bar) | Pt(s) () Pt(s) | Br2(l) | Br-(0.010 M) || H+(0.030 M) | H2(g) (1 Bar) | Pt(s). - 03: Electrochemistry

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NEET-XII-Chemistry

03: Electrochemistry

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Qstn# II-5 Prvs-Qstn Next-Qstn

#5
Write the Nernst equation and emf of the following cells at 298 K:
() Mg(s) | Mg²⁺(0.001M) || Cu²⁺(0.0001 M) | Cu(s)
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Mg(s) | Mg²⁺(0.001M) || Cu²⁺(0.0001 M) | Cu(s)
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
Ans : null () For the given reaction, the Nernst equation can be given as:

= 2.7 - 0.02955

= 2.67 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 2.7 - 0.02955

= 2.67 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

#5-i
Mg(s) | Mg²⁺(0.001M) || Cu²⁺(0.0001 M) | Cu(s)
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
() Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
() Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
() Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
Ans : For the given reaction, the Nernst equation can be given as:

= 2.7 - 0.02955

= 2.67 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

() For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)
() For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)
() For the given reaction, the Nernst equation can be given as:

#5-ii
Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)
Ans : For the given reaction, the Nernst equation can be given as:

= 0.52865 V

= 0.53 V (approximately)

#5-iii
Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)
Ans : For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)

#5-iv
Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).
Ans : For the given reaction, the Nernst equation can be given as: