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Spontaneity

Determine whe...

Question

Determine whether the following reaction will be spontaneous or non-spontaneous under standard conditions.
$Z n (s) + {C u}^{2 +} (a) ⟶ {Z n}^{2 +} (a q) + C u (s) △ H^{0} = - 219 k J, △ S^{0} = - 21 {J K}^{- 1} (S p o n t a n e o u s)$

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Solution

$Δ G = Δ H - T Δ S$
$T = 29$ $K$
$Δ G < 0$ for spontaneous process.
$Δ G = - 219 \times 1000 - [(- 21) \times 298$ $K]$
$⟹ Δ G = - 212.742$ $k J$
Therefore, process is spontaneous.

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Q. Determine whether the following reaction will be spontaneous or nonspontaneous under standard conditions.

Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q) + C u (s), Δ H^{0} = - 219 k J, Δ S^{0} = - 21 J K^{- 1}

Q. A cell is represented by

Z n ∣ ∣ {Z n}^{2 +} (a q) ∣ ∣ ∣ ∣ {C u}^{2 +} (a q) ∣ ∣ C u

{C u}^{2 +} + {2 e}^{-} ⟶ C u, E^{\circ} = + 0.35 V

{Z n}^{2 +} + {2 e}^{-} ⟶ Z n, E^{\circ} = - 0.763 V

. Write the cell reactions, emf of the cell and state whether the cell reaction will be spontaneous or not?

Q. Consider the cell,

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | C u

The standard reduction potentials are

+ 0.35 V

2 e^{-} + C u^{2 +} (a q) \to C u^{2 +} (a q) (1.0 M) | C u

The standard reduction potentials are

+ 0.35 V

2 e^{-} + C u^{2 +} (a q) \to C u

- 0.763 V

2 e^{-} + Z n^{2 +} (a q) \to Z n

Calculate the emf of the cell and tell whether the cell reaction spontaneous or not ?

A l^{3 +} (a q) + 3 e^{-} \to A l (s); E^{\circ} = - 1.66 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{\circ} = + 0.34 V

What voltage is produced under standard conditions to give a spontaneous reactions by combination of these two-half cells?

Q. The standard reduction potential for

Z n^{2 +} / Z n, N i^{2 +} / N i

F e^{2 +} / F e

- 0.76, 0.23

- 0.44 V

, respectively.

X + Y^{2 +} \to X^{2 +} + Y

will be spontaneous when

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