Heat of Neutralisation of strong Acid and strong base is $- 57 K J$ . The amount of heat released when $0.5 m o l e$ of $H N O_{3}$ solution is added to $0.2 m o l e$ of $N a O H$ solution is

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What would be the heat released when an aqueous solution containing 0.5 mole of HNO3 is mixed with 0.3 mole of OH−?Given: Enthalpy of neutralisation is −57.1 kJ

The correct option is C 17.1 kJThe enthalpy of neutralization is −57.1 kJ/mol.0.3 mole of HNO3 will react with 0.3 moles of OH−. H++OH−⟶H2OThe heat released would be 0.3mol×−57.1kJ/mol=17.1kJ

What would be the heat released when an aqueous solution containing $0.5$ mole of $H N O_{3}$ is mixed with $0.3$ mole of $O H^{-}$ ?
Given: Enthalpy of neutralisation is $- 57.1 k J$

The correct option is C $17.1 k J$
The enthalpy of neutralization is $- 57.1 k J / m o l$ .
$0.3$ mole of $H N O_{3}$ will react with 0.3 moles of $O H^{-}$ .

$H^{+} + O H^{-} ⟶ H_{2} O$

The heat released would be $0.3 m o l \times - 57.1 k J / m o l = 17.1 k J$