A reaction of 100mL of 1.35 M HCl and 100mL of 1.76 M NaOH is monitored and the following temperatures were recorded: starting temperature = 24.6 C; and final temperature = 38.8 C.
Calculate the AH of this reaction.

A) -92142
J/Mole
B) -12439.2
J/Mole
C) 876
J/Mole

  for the reaction is 87935 J

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

=

=

As 1 mole of HCl neutralizes 1 mole of NaOH

0.135 moles of HCl will neutralize = 0.135 mole of NaOH

Thus HCl is the limiting reagent.

Q = Heat absorbed by water = ?

m = mass of water = 200 g    (volume of water=200ml, density of wtaer = 1 g/ml)

c = specific heat capacity =

Initial temperature of water = = 24.6°C

Final temperature of water=  = 38.8 °C

Thus heat released by 0.135 moles is = -11871.2 J

heat released by 1 mole is =

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