If -fG- of OH-aq- H2Ol and -AlOH4-aq are -160 kJ mol-1- -250 kJ mol-1 and -1300 kJ mol-1 respectively- then the value of E- of the following cell reaction at 25-C is- OH-aq- H2Ol - -AlOH4-aq - -fG- - -160 kJ mol-1- -250 kJ mol-1 - -1300 kJ mol-1 - - 25-C - - - - - E- - - -4Als - 3O2g - 6H2Ol - 4OH-aq - 4-AlOH4-aq

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Standard XII

Physics

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)

1.32 V

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2.64 V

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0.50 V

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3.98 V

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The correct option is B 2.64 V
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Similar questions

Q. Consider the following reactions.

(a)

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

m o l^{- 1}

(b)

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

m o l^{- 1}

(c)

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

m o l^{- 1}

(d)

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

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for reaction,

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

is 2.73 V.
If

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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

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[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 +}

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and

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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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The correct option is B 2.64 VSolution

The correct option is B 2.64 V
Solution