1--What is the enthalpy change when 40.1 mL of 0.400 M sulfuric acid reacts with 19.5 mL of 0.133 M potassium hydroxide? H2SO4(aq) + 2KOH(aq) -> K2SO4(aq) + 2H2O(l) deltaH° = -111.6 kJ/mol

2--- What mass of Al (26.89 amu) is consumed when 800. kJ of heat are released by the following reaction? 2Al(s) + Fe2O3(s) -> 2Fe(s) + Al2O3(s) deltaH = -850. kJ

3--Calculate deltaH for the following reaction WO3(s) + 3H2(g) -> W(s) + 3H2O(g) using the following equation 2W(s) + 3O2(g) -> 2WO3(s) deltaH = -1685.4 kJ and the heat of formation for H2O(g)

4--What is the enthalpy change when 40.1 mL of 0.400 M sulfuric acid reacts with 19.5 mL of 0.133 M potassium hydroxide? H2SO4(aq) + 2KOH(aq) -> K2SO4(aq) + 2H2O(l) deltaH° = -111.6 kJ/mol

5-A temperature increase of 67.4 K was recorded after 1.500 g of metallic magnesium (24.305 amu) reacted completely with 100.0 mL of 1.00 M aqueous HCl in a non-ideal coffee cup calorimeter with a heat capacity of 16.0 J/K. If the solution has a specific heat capacity of 3.95 J/(g K) and a density of 1.015 g/ml, what is the deltaH for the following reaction in kJ? Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)