Answer:
To calculate the heat released in this reaction, we need to use the formula:
Q = mcΔT
where Q is the heat released, m is the mass of the solution, c is the specific heat capacity of the solution, and ΔT is the change in temperature.
Assuming the density of the solution is 1 g/mL, the mass of the solution is 100 g (50 mL HCl + 50 mL NaOH). The specific heat capacity of the solution can be assumed to be the same as that of water, which is 4.18 J/g°C.
The change in temperature can be calculated as the final temperature minus the initial temperature:
ΔT = 30°C - 22°C = 8°C
Therefore, we have:
Q = (100 g) * (4.18 J/g°C) * (8°C) = 3344 J
The heat released in the reaction is 3344 J.
The value of ΔH for the reaction can be calculated using the formula:
ΔH = -Q/n
where Q is the heat released, and n is the number of moles of limiting reactant used in the reaction. In this case, the limiting reactant is NaOH, and we can calculate the number of moles of NaOH from its concentration and volume:
n(NaOH) = (0.1 L) * (1 mol/L) = 0.1 mol
Therefore, we have:
ΔH = -(3344 J) / (0.1 mol) = -33,440 J/mol
The value of ΔH for the reaction is -33,440 J/mol, which is negative because the reaction is exothermic (heat is released).