What would be the heat released when an aqueous solution containing `0.5 mol` if `HNO_(3)` is mixed with `0.3` mol of `OH^(-1)` (enthalpy of neutralisation is `-57.1 kJ`)A. `28.5 kJ`B. `17.1 kJ`C. `45.7 kJ`D. `1.7 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` if `HNO_(3)` is mixed with `0.3` mol of `OH^(-1)` (enthalpy of neutralisation is `-57.1 kJ`)A. `28.5 kJ`B. `17.1 kJ`C. `45.7 kJ`D. `1.7 kJ`
Answer» Correct Answer - B `0.5 mol HNO_(3)-=0.5 molH^(+)` `H^(+)+OH^(-)toH_(2)O`, `DeltaH=-57.1 kJ` Here `OH^(-)=0.3 mol` Thus, `OH^(-)` is the limiting reactant When `1` mol of `OH^(-)` ions are neutralised heat released` = 57.1 kJ` `0.3` mol of `OH^(-)` ions are neutralised heat released `=57.1xx0.3=17.13 kJ`

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What would be the heat released when an aqueous solution containing `0.5 mol` if `HNO_(3)` is mixed with `0.3` mol of `OH^(-1)` (enthalpy of neutralisation is `-57.1 kJ`)A. `28.5 kJ`B. `17.1 kJ`C. `45.7 kJ`D. `1.7 kJ`

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