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C6H12O6(s)→C3H6O3(s)+C2H5OH(l)+CO2(g) Calculate ΔH∘rxn
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- Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l),CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) ΔH° = −890 kJ2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (l); ΔH°= −10,914 kJ2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) ΔH° = −1453 kJwhich fuel provides the most energy per gram upon combustion and which provides the least? could you please explain this problem19 Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values). H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l), CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) ΔH° = −890 kJ 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (l) ΔHo = −10,914 kJ 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) ΔH° = −1453 kJ Which fuel provides the most energy per gram upon combustion and which provides the least? Group of answer choices CH3OH provides the most energy per gram and CH4 the least. C8H18 provides the most energy per gram and CH3OH the least. CH4 provides the most energy per gram and CH3OH the least. C8H18 provides the most energy per gram and CH4 the least. CH4 provides the most energy per gram and C8H18 the least.
- Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon: C(s) + H2 O(g) ⟶ CO(g) + H2(g).(a) Assuming that coke has the same enthalpy of formation as graphite, calculate ΔH°298 for this reaction.(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst: 2H2(g) + CO(g) ⟶ CH3 OH(g).Under the conditions of the reaction, methanol forms as a gas. Calculate ΔH°298 for this reaction and for the condensation of gaseous methanol to liquid methanol.(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).Using the standard enthalpies of formation (pictured), calculate ΔHº for the following reactions:a) CO2 (g) + 2NH3 (g) → H2O (g) + CO(NH2)2 (g) b) 2CH4 (g) + Cl2 (g) → 2 CH3Cl (g)Calculate ΔH for the reaction: C2H4 (g) + H2 (g) → C2H6 (g), from the following data.
- Consider the following reactions: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) ΔH = -28.0 kJ 3Fe (s) + 4CO2 (g) → 4CO (g) + Fe3O4 (s) ΔH = +12.5 kJ Use the above information to determine the enthalpy change for the following reaction: 3Fe2O3 (s) + CO (g) → CO2 (g) + 2Fe3O4 (s) Question 19 options: A) -59.0 kJ B) 40.5 kJ C) -15.5 kJ D) -109 kJ E) +109 kJCalculate Δ Hrxn for Ca(s) + 1/2 O2(g) + CO2(g) → CaCO3(s) given the following set of reactions: Ca(s) + 1/2 O2(g) →CaO(s) ΔH = −635.1 kJ CaCO3(s) →CaO(s) + CO2(g) ΔH = 178.3 kJUsing the standard enthalpies of formation in the picture, calculate ΔHº for the following reactions:a) 2H2O2 (l) → 2H2O (l) + O2 (g) b) CH4 (g) + Cl2 (g) → CH3Cl (g) + HCl (g) c) HCl (g) + NaOH (s) → NaCl (s) + H2O (l)
- Calculate the enthalpy change for the following reaction: C2H2(g) → 2 C(s) + H2(g) Given the following data: AH = -393.5 kJ/mol C(s) + O2(g) → CO2(g) H2(g) + 1/2 O2(g) → H2O(1) 2 C2H2(g) + 5 O2(g) → 4 CO2(9) + 2 H2O(1) AH = -285.8 kJ/mol AH = -2598.8 kJ/mol Is this reaction endothermic or exothermic?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(1) Use the following reactions and enthalpy changes: N2H4 (1) + O2 (g) → N2 (g) + 2H,O(1); AH = -622.2 kJ H2 (g) + O2 (9) → H2O(1); AH = -285.8 kJ AH = kJ %3DGiven the standard enthalpy changes for the following two reactions: (1) 2C(s) + H₂(g) → C₂H₂ (9) AH° = 226.7 kJ (2) 2C(s) + 2H₂(g) → C₂H₁ (9) ΔΗ° = 52.3 kJ What is the standard enthalpy change for the following reaction? (3) C₂H₂(g) + H2 (9) → C2H4 (9) AH° =? Standard enthalpy change = kJ