1. A student combusts 504.96 grams of ethene gas, C2H4. How many liters of CO2 (g) are produced at a pressure of 0.993 atm and a temperature of 295 K? C2H4 (g) + 3 O2 (g) 2 CO2 (g) + 2 H2O (g)2.Consider: C7H16 (l) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (l) ΔH˚reaction=- 4130 kJ. How much energy is released when 4.000 moles of C7H16, is combusted? 3. Determine ΔHreaction° for: 4H2O (l) + 2 NH3 (g) → 2NO2 (g) + 7H2 (g) using the following two equations: (1) N2 (g) + 3H2 (g) → 2 NH3 (g) ΔH1° = -184 kJ (2) 4NO2 (g) + 8H2 (g) → 2 N2 (g) + 8 H2O (l) ΔH2° = -196 kJ