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Given that, for the reaction H+ (aq) + OH- (aq) H2 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 ΔH1. (2) 0.5 mole of HNO3 in solution is mixed with 0.2 mole of KOH solution; heat released is ΔH2. (3) 200 cm3 of 0.2 M HCI solution is mixed with 300 cm3 of 0.1 M NaOH solution heat released is ΔH3. The correct order for the numerical value of ΔH1, ΔH2, ΔH3 would be?

Given that, for the reaction H+ (aq) + OH- (aq) H2 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 ΔH1.
(2) 0.5 mole of HNO3 in solution is mixed with 0.2 mole of KOH solution; heat released is ΔH2.
(3) 200 cm3 of 0.2 M HCI solution is mixed with 300 cm3 of 0.1 M NaOH solution heat released is ΔH3.
The correct order for the numerical value of ΔH1, ΔH2, ΔH3 would be?
 

Grade:12

1 Answers

Raghuvir
20 Points
5 years ago
In 1st ... 0.25 mol HCl will react wilth 0.25 mol NaOH, so the reaction will be NaOH + HCl ~ H2O + NaCl, so ∆H1=∆H .In 2nd reaction also there is reaction between an strong acid and strong base but 0.5 mol will not have any impact.so ∆H2=∆H. In 3rd also there is same   reaction but 10 milimoles remain in react that will only change pH of Sol. So ∆H1=

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