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Vector Addition

If ΔfGº of OH...

Question

If Δ_fGº of OH^–(aq), H₂O(l) and [Al(OH)₄]^–(aq) are –160 kJ mol^–1, –250 kJ mol^–1 and –1300 kJ mol^–1 respectively, then the value of Eº of the following cell reaction at 25ºC is

यदि OH^–(aq), H₂O(l) तथा [Al(OH)₄]^–(aq) की Δ_fGº क्रमशः –160 kJ mol^–1, –250 kJ mol^–1 तथा –1300 kJ mol^–1 हैं, तो 25ºC पर निम्नलिखित सेल अभिक्रिया के Eº का मान है

4Al(s) + 3O₂(g) + 6H₂O(l) + 4OH^–(aq) → 4[Al(OH)₄]^–(aq)

A

1.32 V

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B

2.64 V

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C

0.50 V

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D

3.98 V

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Solution

The correct option is B 2.64 V
Solution

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Similar questions

Q. Consider the following reactions.

H_{(a q)}^{+} + O H_{(a q)}^{-} = H_{2} O_{(l)}, Δ H = - X_{1}

m o l^{- 1}

H_{2 (g)} + \frac{1}{2} O_{2 (g)} = H_{2} O_{(l)}, Δ H = X_{2}

m o l^{- 1}

C O_{2 (g)} + H_{2 (g)} = C O_{(g)} + H_{2} O_{(l)} - X_{3}

m o l^{- 1}

C_{2} H_{2 (g)} + \frac{5}{2} O_{2 (g)} = 2 C O_{2 (g)} + H_{2} O_{(l)} + X_{4}

m o l^{- 1}

Enthalpy of formation of

H_{2} O_{(l)}

E_{c e l l}^{o}

4 A l (s) + 3 O_{2} (s) + 6 H_{2} O + 4 O H^{-} \to 4 [A l (O H)_{4}^{-}]

△ G_{f}^{o}

O H^{-}

H_{2} O

are - 157 kJ mol

^{- 1}

and - 237.2 kJ mol

^{- 1}

△ G_{f}^{o}

[A l (O H)_{4}]^{-}

x

- x

Q. For the cell reaction

2 {Fe}^{3 +} (aq) + 2 I^{-} (aq) \to 2 {Fe}^{2 +} (aq) + I_{2} (aq) E °_{cell} = 0.24 V at 298 K

The standard Gibbs energy

△ G^{o}

of the cell reaction is:
[Given that Faraday constant F = 96500 C mol–1]

Z n_{(s)} + C u_{(a q)}^{2 +} \to C u_{(s)} + Z n_{(a q)}^{2 +}

Δ_{f} G^{\circ}

C u_{(a q)}^{2 +}

Z n_{(a q)}^{2 +}

^{- 1}

and 147.2 kJ mol

^{- 1}

respectively, then the standard gibbs energy change for the above reaction is:

Enthalpy change for the reaction $H_{(a q)}^{+} + O H_{(a q)}^{-} ⟶ H_{2} O_{(} l) I S - 57.3 k J m o l^{- 1} .$ If 1 L of $0.5 M J N O_{3}$ is mixed with 2L of 0.1 MKOH, the enthalpy change would be

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