Ammonia reacts with oxygen to form nitrogen dioxide and steam, as follows: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) Calculate the enthalpy change of the reaction.

What is the enthalpy change when  2.00 mol of oxygen (O2) react? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ

Determine the enthalpy for the following reaction, given A# (NH3(g)) = -46.1 kJ/mol, AH (NO(g) = +90.3 kJ/mol, and A (H20(g)) = -241.8 kJ/mol. 4NH3(g) + 502(g) →4NO(g) + 6H20(g) AHrxn = ? kJ -1274 kJ/mol -1,996 kJ/mol +1,274 kJ/mol -905.2 kJ/mol -105.4 kJ/mol

Use the thermochemical equations shown below to determine the enthalpy for this reaction: 2 H2O(g) + 2 Cl2(g) →4 HCl (9) + O2(g) ΔΗ xn Information: COCI 2(g) + H2O(l) → CH2Cl2(1) + O2(g) AH = 19 kJ H2O(g) →H2O(l) AH = -44 kJ HCI (g) 1/2 H2(g) +1/2 Cl2(g) AH = 92 kJ CH2Cl2(1) + H2(g) + 3/2 O2(g) → COCI 2(g) + 2 H2O (1) AH=-161k]

Given the following reactions: Fe2O3(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g); ΔH = −28.0kJ 3 Fe(s)+ 4 CO2(g) →4 CO(g) + Fe3O4(s); ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3(s) + CO(g) → CO2(g) + 2 Fe3O4(s) is which of the following? -109 kJ -15.5 kJ +109 kJ -59.0 kJ

What is the enthalpy of reaction, ΔHrxn for the reaction of nitrogen gas with oxygen gas to produce NO2(g), based on the following information? These reactions are not at standard state or at 298 K. N2(g) + O2(g) → 2 NO(g); ΔH = 332.9 kJ2 NO2(g) → 2 NO(g) + O2(g); ΔH = 718.4 kJ Report your answer in kJ to 1 decimal place.

Calcium carbide,CaC2 , is manufactured by the reaction of CaO with carbon at a high temperature. (Calcium carbide is then used to make acetylene.) What is the enthalpy change if 60.0 g of CaO is allowed to react with an excess of carbon? In kj

Consider the following chemical reaction: C3H8(g) + H2(g) to give C2H6(g) + CH4(g)      ΔH° = ?      Calculate the enthalpy change for the reaction above using Hess's law Thermochemical data: H2(g) + 1\2O2(g) to give H2O(l)           ΔH° =-285.8 kJ  ΔH° combustion for CH4(g)                    ΔH° =-890.0 kJ/mol CO2 giving C(s, graphite) + O2(g)         ΔH°= +393.5 kJ ΔH° combustion for C2H6(g)                    ΔH° =-1560.0 kJ/mol ΔH°f for C3H8(g)                                    ΔH° =-103.8 kJ/mol

The enthalpy of formation of H2O(l) is -285.8 kJ/mol. What is the enthalpy change if 1.62 g H2(g) reacts with 9.21 g O2(g) to form H2O(l)?