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What would be the heat released when an ...

What would be the heat released when an aqueous solutions containing 0.5 mole of ` HNO_3` is mixed with 0.3 mole of ` OH^(-)` (enthalpy of neutralization is -57.1 kJ)

A

`28.5 kJ`

B

` 17.1 kJ`

C

` 45.7kJ`

D

` 1.7kJ`

Text Solution

Verified by Experts

The correct Answer is:
C
0.5 mol `HNO_3 = 0.5 mol H^(+) `
and ` 0.3 mol OH^(-)`
` 0.5 H^(+) (aq) +0.3 H^(-) (aq) to 0.5 H_2O (l)`
` Delta H = 0.8 xx 57 .1`
` " " = 45 . 68 kJ`
` " " = 45 . 7kJ`
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Given that, for the reaction H^(+)(aq)+OH*(aq)H_(2)O(I) , , energy released is 57.1 kJ. Three reactions are given as follows 1 0.25 mole of HCI in solution is neutralized by 0.25 mole of NaOH, heat released is DeltaH_(1) . 2. 0.5 mole of HNO_(3) in solution is mixed with 0.2 mole of KOH solution , heat released is DeltaH_(2) . (3) 200cm^(3) of 0.2 M HCI solution is mixed with 300 cm^(3) of 0.1 M NaOH solution heat released is DeltaH_(3) . The correct order for the numerical value of DeltaH_(1),DeltaH_(2),DeltaH_(3) would be