+ H₂O H+ Δ

Part 1.) 4NH3 (g) +502 (g) - -- > 4 NO (g) 6H2O (g)Write the formation reactions for the compounds shown and their enthalpy of formation values. NO is already provided. rxn 1: -- 1/2 N2 (g) + 1/2 O2 (g) > NO ( g) delta H fNO = ?, rxn 2: N2 (g) + H2 (g) - - > NH3 (g) delta HfNH 3 = ?, rxn 3: H2(g) + O2 (g) - > H 20 (g) delta H fH2O = ? In the delta sheet given I found deltaHf NO +91.3 kJ/mol, deltaHfNH3 = 45.9 kJ/mol, deltaHfH2O -241.8 kJ/mol. Part 2.) Using these three formation reactions (rxn) determine the enthalpy of the rxn. deltaHrxn using Hess's law.

Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂ H₂ (-1300. kJ/mol), C2H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction ΔΗ = C₂H₂(g) + 2H₂(g) → C₂H6 (9) kJ

What is the enthalpy change when  1.00 mol of carbon dioxide (CO2) is formed? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ

In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/mol

Given the following data 2 CIF (g) + O₂(g) → Cl₂ O(g) + F₂O(g) 2 CIF3 (9) +202 (g) → Cl₂ O(g) + 3F₂O(g) 2F2 (g) + O₂(g) → 2F₂O(g) calculate A H for the reaction AH= CIF (g) + F2 (g) → CIF3 (9) Submit Answer kJ Try Another Version ΔΗ = 167.4 kJ Δ Η = 341.4 Κ Δ Η = -43,4 kJ item attempt remaining

d The standard enthalpy change for the following reaction is -602 kJ at 298 K. AH° = -602 kJ Mg(s) + 1/2O₂(g) → MgO(s) ΔΗ — What is the standard enthalpy change for the reaction at 298 K? 2 MgO(s) →→→2 Mg(s) + O₂(g) kj Submit Answer Retry Entire Group 9 more group attempts remaining

2CH3OH(g)→2CH4(g)+O2(g),ΔH=+252.8 kJ   For a given sample of CH3OH, the enthalpy change during the reaction is 82.9 kJ . What mass of methane gas is produced?

Enthalpy changes for the following reactions can be determined experimentally: N₂ (g) + 3 H₂(g) → 2 NH3(g) ΔΗ° -91.8 kJ/mol-rxn 4 NH3(g) + 5 O2 (g) → 4 NO(g) + 6 H₂O(g) Δ, A, H = -906.2 kJ/mol-rxn H₂(g) + 1/2 O₂(g) → H₂O(g) A, H° = -241.8 kJ/mol-rxn = Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that cannot be measured directly because the reaction is reactant-favored). 1/2 N₂(g) + 1/2O2(g) → NO(g) kJ/mol-rxn Enthalpy change

What is the enthalpy change if  6.00 mol of oxygen (O2) are formed? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ