2. Methylhydrazine (N₂H3CH3) is a common liquid propellant used in rocket fuels. Look for the standard molar enthalpies of formation of the reactants and products (you may use the uploaded files or search elsewhere for this). Calculate the AH° for the reaction. ° N2H3CH3 (l) + N2O4 ( ---> H₂O(g) + N2 (g) + CO2(g)

Using the given molar enthalpies of formation, determine the change in enthalpy for the combustion of 1 mole of methanol. , AH°; CH3OH (4) =- 238.6 kJ/mol AH°; CO2 (g) = - 110.5 kJ/mol AH°; H2O (g) = – 241.8 kJ/mol 3 CH3OH (e) +02 (g) → CO2 (g) + 2H2O (g)

The first step in the production of nitric acid from ammonia involves the oxidation of NH3. 4 NH3(g) + 5 O₂ (g) → 4 NO(g) + 6 H₂O(g) 2 a Use standard enthalpies of formation from the table below to calculate the standard enthalpy change for this reaction. Species AfH (kJ/mol) NH3(g) -45.90 NO(g) +90.29 H₂O(g) -241.83 Standard enthalpy change Submit = kJ/mol-rxn

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction (show all work):              P4(g) + 10 Cl2(g)  →  4PCl5(s)             ΔH°rxn =  ? Given:               PCl5(s)  →  PCl3(g) + Cl2(g)                ΔH°rxn = +157 kJ              P4(g) + 6 Cl2(g)  →  4 PCl3(g)              ΔH°rxn = -1207 kJ

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* ions; that is, AH H* (aq)]=0. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S Calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits. 010

12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. calorimeter itself.)

An ideal gas sealed in a rigid 3.13-L cylinder, initially at pressure Pi=12.70 atm, is cooled until the pressure in the cylinder is Pf=1.18 atm. What is the enthalpy change for this process?What is the change in internal energy for this process?

When 1.0 mol N204(g) is formed from 2.0 mol NO2(g) under constant pressure (1 atm) at 298 K, please calculate:(a) the reaction enthalpy (ArH) of this reaction according to the standard molar formation enthalpy of NO2(g) and N204(g)at 298 K, +33.85 kJ/mol and +9.66 kJ/mol, respectively.(b) the entropy change in the surrounding. (hint: equal to the heat received by surrounding / temperature of thesurrounding)

Substance SiO,(s) SICLO H,O) HCIE) AH°, (kJ/mol) -910.7 -687.0 -285.83 -92.307 Calculate the standard enthalpy change for the following reaction: SICI4(1) + 2H20(1) → SIO2 (s) + 4HCI (g)