Answer:
0.075881 kJ
Explanation:
The balanced equation for the reaction between [tex]Ba(OH)_{2}{/tex] and HCl is:
[tex]2HCl + Ba(OH)_{2} --- > BaCl_{2} + 2H_{2}O[/tex]
The enthalpy represents the energy that is either absorbed or released during a chemical reaction. It can be estimated experimentally using a calorimeter to measure the change in temperature after the reaction has occurred. The endpoint of the reaction is determined when there is no change in the temperature in the calorimeter.
With the data, we can use the next equation to estimate the heat (enthalpy) absorbed in this reaction.
[tex]Q=m*Cp*delta T[/tex]
Where
Q is heat, m is mass of the reactants and Cp is the specific heat of the products and delta T is the change of temperature.
Mass of the reactants.
We know that molarity is
[tex] M = \frac{Moles}{volume}[/tex]
So [tex]moles=M*volume[/tex]
We can estimate the moles for each reactant as:
[tex] moles of Ba(OH)_{2} = 0.330 M * 0.05 L =0.0165 moles Ba(OH)_{2} [/tex]
[tex] moles of HCl = 0.660 M * 0.05 L =0.033 moles HCl[/tex]
The molecular mass for each reactant is:
[tex]HCl =36.4 \frac{g}{mol}[/tex]
[tex]Ba(OH)_{2} = 171.34 \frac{g}{mol}[/tex]
The mass for each one is
[tex] HCl = 36.4 \frac{g}{mol} * 0.033 moles HCl =1.2012 g [/tex]
[tex] Ba(OH)_{2} = 171.34 \frac{g}{mol} * 0.0165 moles Ba(OH)_{2} =2.8271 g [/tex]
Total mass = 1.2012 g + 2.83 g = 4.0283 g
Cp is the one for the water
[tex]4.186 \frac{J}{g * C}[/tex]
Delta T = 28.16 °C - 23.66 °C = 4.5 °C
Using the equation
[tex]Q=m*Cp*delta T[/tex]
[tex]Q= 4.0283 g * 4.186 \frac{J}{g * C }* 4.5 C =75.88 J [/tex]
The heat absorbed in this reaction is 75.88 J or 0.075881 kJ
