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 =

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.