An unmeasurable change in enthalpy can be calculated using the Hess law. The following is the reaction of methane to ethylene  2 CH4(g) ⇒ C2H4(g) + H2(g)  Calculate the standard enthalpy change (HH°) of the above reaction using the following thermochemical information. CH4(g) + 2 O2(g) ⇒ CO2(g) + 2 H2O(l) ΔH° = -890.3 KJ  C2H4(g) + H2(g) ⇒ C2H6(g) ΔH° = -136.3 KJ  2 H2(g) + O2(g) ⇒ 2 H2O(l) ΔH° = -571.6 KJ  2 C2H6(g) + 7 O2(g) ⇒ 4 CO2(g) + 6 H2O(l) ΔH° = -3120.8 KJ

Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 8 H,S(g)+40,(9)→ Sg(s)+8 H,O(1) olo Round your answer to the nearest kJ, Ar x10 ?

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?

3. Hydrazine, N2H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N2(g) + 2H2(g) → N2H4(l) Use the following reactions, enthalpy changes, and Hess’s Law N2H4(l) + O2(g) → N2(g) + 2H2O(l); ΔrH° = −622.2 kJ H2(g) + ½O2(g) → H2O(l); ΔrH° = −285.8 kJ

Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol

CH4(g)+2 O2(g) +CO2(g)+2 H2O(I), ΔΗ 2 CH4(g) + O2(g) → 2 CH3OH(I), ΔΗ2 5. Express the enthalpy change for the third reaction 2 CH3OH(I) + 3 O2(g) → 2 CO2(g) + 4 H2O(g), ΔΗ3 in terms of ΔΗ1 and ΔΗ2. Ο (Α) ΔΗ3 = ΔΗ1 + ΔΗ2 ) (B) ΔΗ3 = ΔΗ1 -ΔΗ2 Οι ΔΗ3-2ΔΗ-ΔΗ2 Ο (D) ΔHg = 2ΔΗ2 - ΔΗ1 Ο (Ε) ΔΗ3 = 2ΔΗ + ΔΗ2

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

Choose ALL the molecules with zero standard-enthalpy-of-formation (ΔHof)=0) N2(g) H2O(g) K(s) FeCl2(s) Fe(s) C(graphite) O2(g) H2O(l)

When 9.42 g of methane (CH4) is burned in a bomb calorimeter (heat capacity = 2.677 × 103 J/°C), the temperature rises from 24.00 to 27.08°C.  Calculate the enthalpy change for the following reaction.  (C= 12.00 amu, H = 1.00 amu)                                                       CH4(g) + 2O2(g)  →  CO2(g) + 2H2O(l) Group of answer choices a. 8.425 kJ b. –14.01 kJ c. –8.425 kJ d. 8245 J e. 14.00 kJ

Hot water heaters often use natural gas (methane) to generate heat. Methane and oxygen react to form carbon monoxide according to the overall equation: 2CH4(g)+3O2(g) = 2CO(g)+4H2O(g) The enthalpy of formation for each compound are as follows: CH4: - 74.6 O2: 0 CO: - 110.5 H2O: - 285.8 Part A: calculate the overall enthalpy change of the reaction. Part B: A typical water heater contains 40.0 gallons of water. After a long vacation, you come home and turn your water heater from "vacation mode" to hot. How many moles of methane must be combusted to heat the water in your water heater from 30.0°C to 48.0°C? The density of water is 3.79 kg/gal, the specific heat capacity of water is 4.182 J/g°C, and the water heater has a heat capacity of 850.0 J/g°C.