Can someone check my work on this question? Calculate ΔH for the reaction described by the equation. (Hint: Use the value for the approximate amount of heat absorbed by the reaction that you calculated in a previous exercise.)
Ba(OH)2 ⋅ 8H2O(s) + 2NH4SCN(aq) ⟶ Ba(SCN)2(aq) + 2NH3(aq) + 10H2O(l)

• In a previous problem, I determined that the heat absorbed was 1.4 kJ when 3.15 g Ba(OH)2 ⋅ 8H2O(s) was used as part of this reaction.
• Molar mass: Ba(OH)2 * 8H2O:
o (1 Ba * 137.33 g/mol Ba) + 2(15.999 g/mol O + 1.008 g/mol H) + 8(2 H * 1.008 g/mol H + 15.999 g/mol O) = 315.5 g/mol Ba(OH)2 * 8H2O
• 3.15 g * 1 mol/315.5 g = 9.98E-3 mol
• 1.4 kJ/9.98E-3 mol = 140 kJ/mol