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- 67.) For the reaction below, write the mass action expression. Then, calculate ΔG if ΔH is 97.56 kJ/mole and ΔS is -0.2164 kJ/mole at 308 K. 2SO2 (g) + O2 (g) ↔ 2SO3 (g)Calculate the ∆0H when 1 mole of methyl alcohol,CH3OH reacts with O2 and the product of reactions is CO2 and H2O. Hint: Create a chemical balance equation first Data : ∆oHf CH3OH = -238.8 Kj/mol ∆oHf CO2 = -393.5Kj/mol ∆oHf H2O = -285.9 Kj/molCalculate ∆Horxn for the following reaction 2H2O2(l) 2H2O(l) + O2(g)given that ∆Hof [H2O(l)] = -285.8 kJ/mol and ∆Hof [H2O2(l)] = -187.6 kJ/mol.
- Carbon dioxide from the atmosphere “weathers”, or dissolves, limestone, CaCO3 by thereaction.CaCO3 (s) + CO2 (g) + H2O (l) → Ca2+ (aq) + 2 HCO3- (aq)What is DH° for this reaction? DH°f CaCO3 (s) = -1206.9 kJ/mol, DH°f CO2 (g) = -393.5 kJ/mol,DH°f H2O (l) = -285.8 kJ/mol, DH°f Ca2+ (aq) = -542.8 kJ/mol, DH°f HCO3 (aq) = -692.0 kJ/molAnswer the problem using the rubrics below as a guide: Given and Asked - Complete data and proper units and significant figures (SF). Equation or formula used - Necessary equations needed in solving the problem are shown. Solution -Complete and organized solution/s shown Correct answer with correct significant figures (SF) and unit. Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O (g) ⇌ H2 (g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations, at a temperature of 760°C? CH4 = 0.126 M H2O = 0.242 M CO = 0.126 M H2 = 1.15 MIn the reaction below, ΔH°f is zero for ________. Ni (s) + 2CO (g) + 2PF3 (g) → Ni(CO)2(PF3)2 (l)
- Liquid carbon disulfide burns in the presence of oxygen to produce two gaseous combustion products, carbon dioxide and sulfur dioxide. Species DHf° (kJ/mol) DGf° (kJ/mol) CS2 (g) 117.4 65.3 CS2 (l) 89.7 65.3 O2 (g) 0.00 0.00 CO2 (g) - 393.5 - 394.4 SO2 (g) - 296.9 - 300.4 Write a balanced equation for this reaction. 2. Calculate the values of ΔH°rxn and ΔG°rxn for this reaction 3. Is this reaction exothermic or endothermic? Liquid carbon disulfide is vapourised to gaseous carbon disulfide. Calculate the value of ΔS°vap for of liquid carbon disulfide at 25°__C₅H₁₂ + __O₂ --> __H₂O + __CO₂ To balance the attached reaction, what coefficient needs to be put in front of the H₂O?What is the value of ∆G°(kJ mol–1 ) for this reaction at 175.4 oC ? The data refer to 25 oC: 2 NO(g) + Cl2(g) ⟶ 2 NOCl(g) Substance NO(g) Cl2(g) NOCl(g) ∆H°f (kJ mol–1) 90.29 0 51.71 ∆G°f (kJ mol–1) 86.60 0 66.07 S° (J K–1 mol–1) 210.65 223.0 261.6 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Calculate ΔG in kJ•mol-1 at 298 K for the following reaction: under the following conditions: (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) P(A) = 0.397 atm, P(AB) = 0.792 atm 2 A(g) + B2(s) → 2 AB(g) ΔGo = -182 kJ•mol-1 The redox reaction below has a ΔG° value of 209. kJ. Determine the standard cell potential(E°cell) for…