Use the values of in Appendix B to calculate the standard free-energy change for the synthesis of dichloroethane from ethylene and chlorine:
Is it possible to synthesize dichioroethane from gaseous
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Chapter 18 Solutions
CHEMISTRY-MOD.MASTERING (18W)
- Using a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.arrow_forwardFrom the data given in Appendix I, determine the standard enthalpy change and the standard free energy change for each of the following reactions: (a) BF3(g)+3H2O(l)B(OH)3(s)+3HF(g) (b) BCl3(g)+3H2O(l)B(OH)3+3HCl(g) (c) B2H6(g)+6H2O(l)2B(OH)3(s)+6H2(g)arrow_forwardHydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine makes for an easily replaceable substituent, these bromine precursors are a necessary part of a vast amount of organic synthesis. Calculate the reaction enthalpy for the synthesis of HBr according to H2(g) + Br2(1) - 2HBr(g) Use the following information: NH3(g) + HBr(g) - NH,Br(s) AH = - 188.32 kJ N2(g) + 3H2(g) - 2NH3(g) AH° = -92.22 kJ N2(g) + 4H2(g) + Br2(1) - 2NH,Br(s) AH = -541.66 kJ a. AH° = -826.08 kJ/mol b. AH = 72.8 kJ/mol c. AH° = -1010.52 kJ/mol d. AH = -257.24 kJ/mol e. AH° = -72.8 kJ/molarrow_forward
- 19 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)arrow_forwardThe industrial synthesis of chloroform by the reaction of methane with Cl2 is carried out according to the following reaction equation:CH4 (g) + Cl2 (g) → CHCl3 (l) + HCl (g)Using the thermodynamic data provided, calculate Ho (in Kj/mol) for this reaction.arrow_forwardThe industrial synthesis of chloroform by the reaction of methane with Cl2 is carried out according to the following reaction equation: CH4 (g) + Cl2 (g) → CHCl3 (l) + HCl (g) Using the thermodynamic data provided, calculate DHo (in Kj/mol) for this reaction.arrow_forward
- 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.arrow_forwardCalculate ΔH for the reaction: C2H4 (g) + H2 (g) → C2H6 (g), from the following data.arrow_forwardChloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) → 3 HCl(g) + CHCl3(g) Calculate ΔrH°, the enthalpy change for this reaction, using the enthalpies of formation of CO2(g), H2O(ℓ), CHCI3(g) (ΔfH° = -103.1 kJ/mol), and the enthalpy changes for the following reactions: CH4(g) + 2 O2(g) → 2 H2O(ℓ) + CO2(g) ΔrH° = -890.4 kJ/mol-rxn 2 HCl(g) → H2(g) + Cl2(g) ΔrH° = +184.6 kJ/mol-ransarrow_forward
- Calculate ΔrG∘ for the following reaction:4CO(g)+2NO2(g)→4CO2(g)+N2(g).Use the following reactions and given ΔrG∘values:2NO(g)+O2(g)→2NO2(g), ΔrG∘= - 72.6 kJmol−12CO(g)+O2(g)→2CO2(g), ΔrG∘= - 514.4 kJmol−11/2 O2(g)+1/2 N2(g)→NO(g), ΔrG∘= 87.6 kJmol−1 Express your answer using one decimal place.arrow_forwardCalculate ΔHrxn for the following reaction: BaO(s)+CO2(g)→BaCO3(s) Use the following reactions and the given values of ΔH for them: Ba(s)+CO2(g)+1/2O2(g)→BaCO3(s), ΔH=-826.5kJ 2Ba(s)+O2(g)→ 2BaO(s), ΔH= -1184.0 kJarrow_forwardCalculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+1/2O2(g)→CaCO3(s) , ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ Express your answer using four significant figures.arrow_forward
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