Calculate ΔH for this reaction N2H4 (l) + O2 (g) → N2 (g) + 2H2O (l) given the following data: Equation ΔH(KJ) 2NH3 (g) + 3N2O (g) → 4N2 (g) + 3H2O (l)  -1010 N2O (g) + 3H2 (g) → N2H4 (l) + H2O (l) -317 2NH3 (g) + 1/2O2 (g) → N2H4 (l) + H2O (l)  -143 H2 (g) + 1/2O2 (g) → H2O (l)  -286

The compound WO3(s) is utilized in the refining process of tungsten from its mineral ore. Tungsten can be produced as follows: Reaction 1: WO3(s) + 3H2(g) → W(s) + 3H2O(g) a) From the following data calculate the enthalpy of the above reaction Reaction 2: 2W(s) + 3O2(g) → 2WO3(s)          ΔH = –1685.4 kJ Reaction 3: 2H2(g) + O2(g) → 2H2O(g)            ΔH = –477.84 kJb) Estimate the change of internal energy for Reaction 1. c) Is Reaction 1 exothermic or endothermic?

Ethanol can be made from the fermentation of crops and has been used as a fuel additive to gasoline.         C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)   Part B Calculate ΔrH∘ (The standard enthalpy of formation of liquid ethanol is −277.6 kJmol−1, of gaseous carbon dioxide is −393.5 kJmol−1, and of gaseous water is −241.8 kJmol−1.) Express your answer in kilojoules per mole to one decimal place.

A chemist measures the enthalpy change AH during the following reaction: 2 H,O(1) + O2(9)→2 H,O2(1) ДН-196. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 4H, 0, (1) → 4H,0(1) + 20, (g) kJ 2H,0, (1) → 2H,0(1) + 0, (g) I kJ 1 H,0(1) + 0,(2) - H,0,) H,0, (1) O kJ