The synthesis of ethanol from ethylene and water proceeds according to the reaction C2H4(g) + H2O(1) = C2H5OH(1) where \Delta G\deg rxn = -116.6 kJ/mol. If the pressure of the vessel is 251 atm at 580 K, the Gibbs free energy is kJ/mol. (Watch units. Report answer to 1 decimal place and canvas will round where appropriate.)
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- Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process. Question: What is the change in the system's energy during this reaction? How would your answer differ if the H2O ended up as liquid water instead of vapor?Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process. Question: How much heat is given off during this reaction, assuming that no "other" forms of work are done?Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process. Question: What is ΔH for the actual reaction in which methane and oxygen form carbon dioxide and water vapor directly? Explain.
- Construct enthalpy cycles; use Hess's law and the following data to calculate the enthalpy of formation of ethane (from carbon and hydrogen gas). Cis) + Ozig) + CO2(g) AHa = -394kJmol H2g) + %02(a) – H20 m AH°. = -286kJmol1 + 3%O2(g) → 2002(9) + 3H20 m AH = -1560kJmol1Determine the enthalpy change, AH°, for the following reaction%3B N2(g) + 2H2(g) N2H4() Given the following thermochemical equations. 2H2O(1) + N2(g) N2H4() + O2(g) → H2(g) + ½ O2(g) → H20() ΔΗ? AH° = -285.9 kJ -> AH° = - 622.0 kJ %3D +50.2 kJ -236.2 kJ +106.1kJ 0 kJ -151.7 kJ OO OOOThe vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. $$H2O(l)+40.7kJH2O(g)Assume that at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80 mL and 30.62 L, respectively. a. Calculate the work done on or by the system when 1.25 mol of liquid H2O vaporizes. answer in J. b. Calculate the water's change in internal energy. answer in kJ.
- Q\4: Combustion 0.1 mole of propane in bomb calorimeter with excess amount of oxygen represented by reaction C3H8 (g) +50₂ (g) → 3C0₂(g) + 4H₂0 (1) If initial temp. of calorimeter was 25 C° & total thermal capacity 97.1 KJ.C-1. The reaction leaded temp. rose to 27.282 C°. Determine AH & AE in unit of 1 mole C3H8 KJANADARD ENTHAL FORMAT X "0/c/NDA5MzgwMzl1MDA3/a/NDQyMTg5MDEyNTgz/details 2407599116051397577_n.png Open with - Standard Enthalpy of Formation and Reaction The thermite reaction involves aluminum and iron(III) oxide 2Al(s) + Fe,03(s) → Al203 (s) + 2Fe(1) This reaction is highly exothermic, and the liquid iron formed is used to weld metals. Calculate the heat released in kilojoules per gram of Al reacted with Fe,03. The AH for Fe() is 12.40 kJ/mol and AH° for Fe,0, is -822.2 kJ/mol. The molar mass of Al is 26.98g. +What is AG (in kJ) for 2 SO2(g) + O2(g) – 2 S03(g) at 700 K, under standard conditions of 1 bar partial pressure for all gases, given that K = 3.0×10“ at 700 K? O -60. +36 0.0 +60. -36
- Trouton's rule states that the molar enthalpy of Chemical AHvap Boiling AHfus Compound vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion-ion attractions is given by formula (kJ-mol-1) point (K) (kJ-mol¬1) chloromethane CH;CI 21.40 249.06 6.43 AH vap (85 J. K-1. mol-') To H,0 water 40.65 373.15 6.01 where T, is the normal boiling point of the liquid hydrogen H,S 18.67 213.60 18.67 in kelvins. sulfide Apply Trouton's rule to estimate the value of AHvap for these compounds. chloromethane: AHvap kJ/molWhat is the standard enthalpy of formation of liquid n-butanol, CH3CH2CH2CH20H? CH3CH2CH2CH20H(1) + 602(g) - 4CO2(g) + 5H20(1) AH° = -2675 kJ CO2(g) AH°f (kJ/mol) - 393.5 H20(1) AH°F (kJ/mol) - 285.8 O a. -1996 kJ O b. +3355 kJ O C. -3355 kJ o d. -328 kJ O e. +328 kJThermo- Problem 4.23 At 298 K. AH; 131.28 kJ-mol for the reaction -1 with Cp.-8.53, 33.58, 29.12, and 28.82 J K mol for graphite, H₂O(g). CO(g), and H₂(g), respectively Part A Calculate AH; at 210 *C from this information. Assume that the heat capacities are independent of temperature. Express your answer to five significant figures and include the appropriate units. ΔΗ: (210 °C) - Submit Provide Feedback HÅ Value Request Answer Units C(graphite) + H₂O(g) → CO(g) + H₂(g)