What would be the heat released when an aqueous solution containing 0.5 mol of HNO_(3) is mixed with 0.3 mol of OH^(-) (enthalpy of neutralisation is -57.1 kJ)?

What would be the heat released when an aqueous solution containing 0.

1.	What would be the heat released when an aqueous solution containing 0.5 mol of HNO_(3) is mixed with 0.3 mol of OH^(-) (enthalpy of neutralisation is -57.1 kJ)?
Answer» `28.5 kJ` `17.1 kJ` `45.7 kJ` `1.7 kJ` Solution :0.5 MOL `HNO_(3) equiv 0.5 mol H^(+)` `H^(+) + OH^(-) to H_(2)O`,`DELTAH = -57.1 kJ` Here `OH^(-) = 0.3 mol` . Therefore, `OH^(-)` is the limiting reactant. When 1 mol of `OH^(-)` ions are NEUTRALISED, heat released = 57.1 kJ For 0.3 mol of `oh^(-)` ions, heat released `= 57.1 XX 0.3= 17.13` kJ