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  • Please refer to the given set of reactions with the respective enthalpy change <img alt="i. \: H(g)+Cl(g)\rightarrow HCl(g)\: \: \: \:\: \: \: \: \: \: \: \: \Delta H_1=-430kJ" src="https

Please refer to the given set of reactions with the respective enthalpy change

i. \: H(g)+Cl(g)\rightarrow HCl(g)\: \: \: \:\: \: \: \: \: \: \: \: \Delta H_1=-430kJ

ii. \: HCl(g)+aq\rightarrow H^\oplus(aq) +Cl^\ominus (aq)\: \: \: \: \: \: \: \Delta H_2=-80kJ

iii. \: H(g)\rightarrow H^\oplus +e^-\: \: \: \:\: \: \: \: \: \: \: \: \Delta H_3=1320kJ

iv. \: Cl(g)+e^-\rightarrow Cl^\ominus (g) \: \: \: \:\: \: \: \: \: \: \: \: \Delta H_4=-350kJ

Find the enthalpy of hydration of HCl

H^\oplus (g)+Cl^\ominus (g)+aq\rightarrow H^\oplus (aq)+Cl^\ominus (aq)

 

Option: 1

+1480 KJ

 


Option: 2

-1480 KJ


Option: 3

-2180 KJ


Option: 4

+2180 KJ


Answers (1)

best_answer

If we add reactions i and ii and subtract iii and iv from it, then we will get the resultant reaction which is same as hydration enthalpy of HCl.

H^\oplus (g)+Cl^\ominus (g)+aq\rightarrow H^\oplus (aq)+Cl^\ominus (aq)

\Delta H=\Delta H_1+\Delta H_2-\Delta H_3-\Delta H_4

\Delta H=-430-80-(1320)-(-350)

\Delta H=-1480KJ

Hence, option number (2) is correct

Posted by

Sayak

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