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in Chemical thermodynamics by (64.7k points)
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100 ml 0.5 N H2SO4 (strong acid) is neutralised with 200 ml 0.2M NH4 OH in a constant pressure Calorimeter which results in temperature rise of 1.4°C. If heat capacity of Calorimeter content is 1.5 kJ/°C. Which statement is /are correct Given:

HCl+ NaOH →NaCl +H2+ 57 kJ

CH3COOH NH4OH → CH3COONH4+ H2O +48.1 kJ

(A) Enthalpy of neutralisation of HCl v/s NH4 OH is -52.5 kJ/moL

(B) Enthalpy of dissociation (ionization) of NH4 OH is 4.5 kJ/moL

(C) Enthalpy of dissociation of CH3COOH is 4.6 kJ/mol

(D) ΔH for 2H2O(l) →2H (aq) +2OH- is 114 kJ.

1 Answer

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Best answer

Correct option (A, B, D)

Explanation:

H2SO4 + 2(NH4)OH → (NH4 )2SO4 + 2H2O

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