Calculate the dissociation constant of NH4OH at 298 K- if H- and - S- for the given changes are as follows- NH3-H-NH4- - H-52-2 kJ mol-1- - S-1-67 J K-1 mol-1 H2O - H- -OH- - H-56-6 kJ mol-1- - S- - -76-53 J K-1 mol-1

The correct option is A K_b = 1.7× 10^ 5 #160; NH_3+H^⊕ #160;⇌ #160;⊕NH_4; #160;Δ H^⊝= 52.2 Adding, #160; #160; #160; #160; #1 ...

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Gibbs Free Energy & Spontaneity

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Question

Calculate the dissociation constant of $N H_{4} O H$ at 298 K, if $△ H^{⊝}$ and $Δ S^{⊝}$ for the given changes are as follows:
$N H_{3} + H^{\oplus} ⇌ \oplus N H_{4}$ ;

$Δ H^{⊝} = - 52.2 k J m o l^{- 1}, Δ S^{⊝} = 1.67 J K^{- 1} m o l^{- 1}$

$H_{2} O ⇌ H^{\oplus} + ⊝ O H; Δ H^{⊝} = 56.6 k J m o l^{- 1}$ ;

$Δ S^{⊝} = - 76.53 J K^{- 1} m o l^{- 1}$

K_{b} = 1.7 \times 10^{- 5}

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K_{b} = 1.7 \times 10^{- 3}

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K_{b} = 1.7 \times 10^{- 1}

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K_{b} = 3.4 \times 10^{- 5}

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