The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, ΔH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. Reaction 1: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g),C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), ΔH1=−2043 kJΔ�1=−2043 kJ Reaction 2: 3C3H8(g)+15O2(g)→9CO2(g)+12H2O(g),3C3H8(g)+15O2(g)→9CO2(g)+12H2O(g), ΔH2=?

Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D

Given the two thermochemical equations below, find the enthalpy change for the reaction:         N2H4 (l)  +   H2 (g)    →    2 NH3 (g)          delta H =  ?        Given:             N2O4 (g)  +  3 H2 (g)    →     2 NH3 (g)  +  2 O2 (g)      delta H =   – 100.96 kJ             N2O4 (g)  +  2 H2 (g)    →     N2H4 (l)  +  2 O2 (g)        delta H =   + 41.47 kJ Select one: a. – 142.43 kJ b. – 59.49 kJ c. + 41.47 kJ d. + 59.49 kJ e. + 142.43 kJ f. none of these g. – 100.96 kJ

For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole of C8H18(g)consumed, under standard conditions.   C8H18(g)+25/2O2(g)⟶8CO2(g)+9H2O(g)  Δ?∘rxn=−5104.1 kJ/mol What is the standard enthalpy of formation of this isomer of C8H18(g)?

Analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, ΔH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2.

Calculate the enthalpy of formation of 1 mole SO₂(g) from the standard enthalpy changes of the following reactions: 2SO3(g)2SO₂(g) + O₂(g) 2S (s) +30₂(g) → 2SO3(g) →→ SO₂(g) S(s) + O₂(g) kJ ΔΗ AH rxn 1=+196 kJ rxn 2 = -790 kJ AHO rxn 3 = ? k

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.

（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g)     ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A?   （2）Consider the reaction: C (s) + O2 (g) → CO2 (g)     ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?

For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole of C8H18(g) consumed, under standard conditions. C8H18(g)+(25/2) O2(g)⟶8CO2(g)+9H2O(g)  Δ?∘rxn=−5104.1 kJ/mol   What is the standard enthalpy of formation of this isomer of C8H18(g)?

Using Enthalpies of formation provided on the exam determine the change in enthalpy (kJ/mol) for the following reaction.  Do not type units into your answer.   CH4(g) + 2 O2(g) ⟶⟶ CO2(g) + 2 H2O(l)     Δ?=?ΔH=?