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

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

is there any options? maybe im just not seeing them but i need the options to

-love shrooms