Consider an amphoteric hydroxide, M ( OH ) 2 ( s ) , where M is a generic metal. M ( OH ) 2 ( s ) − ⇀ ↽ − M 2 + ( aq ) + 2 OH −
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Answer: 54.4 kJ/mol
Explanation:
First we have to calculate the moles of HCl and NaOH.
The balanced chemical reaction will be,
From the balanced reaction we conclude that,
As, 1 mole of HCl neutralizes by 1 mole of NaOH
So, 0.05 mole of HCl neutralizes by 0.05 mole of NaOH
Thus, the number of neutralized moles = 0.05 mole
Now we have to calculate the mass of water:
As we know that the density of water is 1 g/ml. So, the mass of water will be:
The volume of water =
Now we have to calculate the heat absorbed during the reaction.
where,
q = heat absorbed = ?
= specific heat of water =
m = mass of water = 100 g
= final temperature of water =
= initial temperature of metal =
Now put all the given values in the above formula, we get:
Thus, the heat released during the neutralization = 2.72 KJ
Now we have to calculate the enthalpy of neutralization per mole of :
0.05 moles of releases heat = 2.72 KJ
1 mole of releases heat =
Thus the enthalpy change for the reaction in kJ per mol of HCl is 54.4 kJ