From the following data, mark the option(s) where $Δ H$ is correctly written for the     given reaction.
Given: $H^{+} (a q) + O H^{-} (a q) \to H_{2} O (l); Δ H = - 57.3 k J$
                                                 $Δ H_{s o l u t i o n} o f H A (g) = - 70.7 k J / m o l$
                                                 $Δ H_{s o l u t i o n} o f B O H (g) = 20 k J / m o l$
             $Δ H_{i o n i z a t i o n} o f H A = 15 k J / m o l a n d B O H$ is a strong base
Reaction $Δ_{r} H (k J / m o l)$
A) $H A (a q) + B O H (a q) \to B A (a q) + H_{2} O$ - 42.3
B) $H A (g) + B O H (g) \to B A (a q) + H_{2} O$ -93
C) $H A (g) \to H^{+} (a q) + A^{-} (a q)$ - 55.7
D) $B^{+} (a q) + O H^{-} (a q) \to B O H (a q)$ -20

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answer is A, B, C.

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Detailed Solution

a) $Δ H = 15 + 0 - 57.3 = - 42.3 k J$

b) $H A + B O H \to B A + H_{2} O$

c) $Δ H = - 70.7 + 15 = 55.7$

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