Which of the following reactions will have the value of enthalpy of neutralisation as $- 57.1 k J m o l^{- 1}$ ?

C H_{3} C O O H + N a O H \to C H_{3} C O O N a + H_{2} O

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H C I + N a O H \to N a C I + H_{2} O

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H C I + N H_{4} O H \to N H_{4} C I + H_{2} O

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H C O O H + N a O H \to H C O O N a + H_{2} O

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Solution

The correct option is C $H C I + N a O H \to N a C I + H_{2} O$
According to experimental data, Enthalpy of neutralisation is -57.1 kJ $m o l^{- 1}$ for a strong acid and a strong base (This value to be remembered).

Suggest Corrections

Similar questions

\to

H C l + N a O H ⟶ N a C l + H_{2} O; Δ H = - 57.1 k J m o l^{- 1}

Δ H

H C l

N a O H

C H_{3} C O O H + N a O H ⟶ C H_{3} C O O N a + H_{2} O . . . . Δ H = - 13.2 K c a l

H^{\oplus} + ⊖ O H ⟶ H_{2} O; . . . . Δ H = - 13.7 K c a l

N H_{4} O H

H C l + N H_{4} O H ⟶ N H_{4} C l + H_{2} O; Δ H = - 12.27 K c a l

What are the products of the reaction, $C H_{3} C O O H + N a_{2} C O_{3} \to$ ?

B + N a O H \to 2 N a_{3} B O_{3} + H_{2}

P_{4} + N a O H + H_{2} O \to N a H_{2} P O_{2} + P H_{3}

S + N a O H \to N a_{2} S_{2} O_{3} + N a_{2} S + H_{2} O

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