The heat of reaction is -6.7 KJ/mol.
The equation of the reaction is;
3H2SO4(aq) + 2Al(OH)3 ------> Al2(SO4)3(s) + 6H2O(l)
Number of moles of H2SO4 = 66.667/1000 L × 3.000 M = 0.2 moles
Number of moles of Al(OH)3 = 66.667/1000 L × 4.000 M = 0.27 moles
If 3 moles of H2SO4 reacts with 2 moles of Al(OH)3
0.2 moles of H2SO4 reacts with 0.2 moles × 2 moles/3 moles = 0.13 moles
We can see that there is more than enough Al(OH)3 hence H2SO4 is the limiting reactant.
Temperature change = 24.7°C - 22.3°C = 2.4°C
Heat capacity of the coffee cup = 1.10 J/g C
Total volume of solution = 66.667 mL + 66.667 mL = 133.334 mL
Mass of solution = 133.334 g
Density of solution = 1 g/ml
Specific heat capacity of solution = 4.18 J/g C
Total heat released =- (Heat absorbed by calorimeter + Heat absorbed by solution)
Total heat released = -[(1.10 J/g C × 2.4°C) + (133.334 g × 4.18 J/g C × 2.4°C)]
Total heat released = -1.34 KJ
Heat of reaction = -1.34 KJ/0.2 moles = -6.7 KJ/mol
Learn more: https://brainly.com/question/4147359
