inside a calorimeter, 0.0075g of sodium hydroxide reacts with 100.0 ml of 0.1500 M sulfuric acid. the initial temperature of the resulting 100.01g solution was 19.67 celcius and it reached a peak of 34.06 celcius. calculate the ethalphy change for this neutralization reaction and write a balanced thermochemical equation.

when 24.0g of carbon and 10.0g of hydrogen are placed in a bomb calorimeter and reacted to according to the equation 3C (g) + 4H2(g)  = C?H?.(propane) (g) + 103.8kJ, the maxium amount of heat liberated by this reaction is 

Predict the change in enthalpy due to the combustion of 10.0 g of propane. Assuming that the molar heat of combustion of propane is -2043.9 kJ/mol.

Use the calorimeter data for the combustion of magnesium to determine the molar enthalpy of reaction (in kJ/mol)  for magnesium

Mass of Mg(s) 0.31 g

Initial temperature of calorimeter contents 23.6 ºC

Final temperature of calorimeter contents 36.8 ºC

Volume of calorimeter 100mL

I'm not sure what to do with the Volume. 

Given the reaction

3 NO₂(g)   +   H₂O(l)   →   2 HNO₃(l)   +   NO(g)   Δ_rH = -72.0 kJ,

calculate the molar enthalpy of reaction, _rH for:

          3)  H₂O(l)