For the rxn l₂(g) -> 1₂(s), AH = -62.4kJ at 25C, based on these data, at 25C a) AHvap = 62.4 kJ b)AHvap = 62.4 kJ c)AHsub= -62.4 kJ d) AHsub= 62.4 kJ
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- At 381 K, the following reaction takes place: Hg2Cl4(g) + Al2Cl6(g) --> 2 (HgAlCl5)(g) ΔH = +10 kJ (a) Offer an explanation for the very small ΔH for this reaction for the known structures of the compounds. (img 1) (b) Explain why the small ΔH in this reaction is evidence against (img 2) as the structure of Hg2Cl4(g).Calculate the free energy change (ΔG) in kJ for the following reaction at 75°C with a ΔH°rxn of -2217 kJ and a ΔS of 101.1 J/K. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Report your answer to the closest kJ. Do NOT include units.Given the standard heats of formation for the following compounds, calculate the ΔH° heat of reaction, for the following reaction: Fe3O4(s) + CO(g) ---> 3 FeO(s) + CO2(g) ΔHf° for Fe3O4 = -1118 kJΔHf° for CO = -110.5 kJΔHf° for FeO = -272 kJΔHf° for CO2 = -393.5 kJ
- Determine AGrxn for 2 A(g) + B₂(g) → 2 AB(g) A. -400 kJ B. -250 kJ C. -200 kJ D. -100 kJ E. -50 kJ Compound(state) AG (kJ/mol) A(g) B₂(g) AB(g) 0 -100 -150Given the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)Estimate ΔG° rxn for the following reaction at 449.0 K. CH 2O( g) + 2 H 2( g) → CH 4( g) + H 2O( g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K
- Determine ΔH°rxn at 25 °C for the reaction2 NOCl(g) → N2(g) + O2(g) + Cl2(g)given that the standard heat of formation (ΔH°f) of NOCl(g) is 51.7 kJ/mol -51.7 kJ -103.4 kJ 51.7 kJ 25.9 kJ -25.9 KJ 103.4 kJCalculate delta H for the following rection, FeO + CO = Fe + CO2 from the following data: Fe2O3 + 3CO --> 2Fe +3CO2 Delta H= -23 kJ 3Fe2O3 + CO --> 2Fe3O4 +CO2 Delta H= -39 kJ Fe3O4 +CO --> 3FeO +CO2 Delta H= +18 kJWhat is the entropy at SATP of a reaction where ∆Hºrxn=-12.5 kJ and Keq=32.1? -0.150 J/K -150 J/K -29.4 J/K -13.1 J/K
- Estimate ΔG°rxn for the following reaction at 307 K.CH4(g) + 2 O2(g) → CO2 (g) + H2O (l) ΔH°= -890.4 kJ; ΔS°= -242.2 J/K +816.0 kJ +66.3 kJ -66.3 kJ -816.0 kJ -250 kJ8. Given the standard heats of formation for the following compounds, calculate the ΔH° heat of reaction, for the following reaction: Fe3O4(s) + CO(g) ---> 3 FeO(s) + CO2(g) ΔHf° for Fe3O4 = -1118 kJΔHf° for CO = -110.5 kJΔHf° for FeO = -272 kJΔHf° for CO2 = -393.5 kJ Please show work3. A reaction has a standard free energy change (G⁰) of -21.6 kJ/mol at 25 ⁰C.a. Is this reaction spontaneous or non-spontaneous at 25 ⁰C? b. Given the value of G⁰ above (-21.6 kJ/mol), what is the value of the equilibrium constant (K or Keq)for this reaction at 25 ⁰C?