20.5) Calculate ΔGo for the reaction SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) Substance SiCl4&nbs
The combustion of propane, C3H8, occurs via the reaction C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) C3H8 (g)= -104.7 CO2(g)= −393.5 H2O(g)= −241.8 Calculate the enthalpy for the combustion of 1 mole of propane.
Calculate rxn for the below combustion reaction, determine if entropy increases or decreases. Assume 1 mol of substance at 25 Celsius. C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) Delta G of C3H8 = -23.4 kj/mol Delta G of O2 = 0 kj/mol Delta G of CO2 = -394.36 kj/mol Delta G of H2O = -237.1 kj/mol We were unable to transcribe this imageWe were unable to transcribe this image
Propane (C3H8)burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxnΔ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/molkJ/mol.) Express the enthalpy in kilojoules to four significant figures.
Please help? Calculate deltaHr for the reaction: C3H8(g) + 5O2(g)----->3CO2(g) + 4H2O(l) Given: 3C(s) + 4H2(g)----->C3H8(g) deltaH -24.8 kcal H2(g) + 1/2 O2(g)----->H2O(l) deltaH -68.3kcal C(s) + O2(g)-------> CO2(g) deltaH -94.0 kcal
Must Show all work Calculate S deg for the reaction: 1/2SiCl4(g) + Mg(s) --------> MgCl2(s) + 1/2 Si(s) Substance: SiCl4(g) Mg(s) MgCl2(s) Si(s) S deg (J/K x mol): 330.73 32.68 89.62 18.83
Consider the following reaction: SiCl4(g) ⇌ Si(s) + 2Cl2(g) The initial partial pressure of SiCl4 is 1.00 atm. At equilibrium, the total pressure is 1.35 atm. Calculate Kp for this reaction. Report your answer to the correct number of significant figures.
Consider the following balanced reaction: 3C(s) +4H_2(g) rightarrow C3H8(g) Calculate given the following information. SHOW YOUR WORK. H_2(g)+v2o2 rightarrow HO deltaH0= -285.8 kJ C(s) + O2 rightarrow CO2 deltaH0 =-393.5 kJ C3H8(s) + O, rightarrow 3CO2+ 4H_20 deltaH0 = -2219.9 kJ
1At a certain temperature, 659 K, Kp for the reaction, N2O4(g) <=> 2 NO2(g), is 5.4 x 10-69. Calculate the value of DGo in kJ for the reaction at 659 K. 2Given the values of So given below in J/mol K and the values of ΔHfo given in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of propane to form carbon dioxide and gaseous water at 298 K. S (C3H8(g)) = 271 S (O2(g))...
Calculate the standard entropy change for the reaction2Mg(s)+O2(g)→2MgO(s)using the data from the following table:Substance△ Hf (kJ/mol)△Gf (kJ/mol)S0 [J/(K/mol)]Mg(s)0.000.0032.70O2(g)0.000.00205.0MgO(s)-602.0-569.627.00Express your answer to four significant figures and include the appropriate units.
Using the data in the table calculate ΔGo (Delta Go) and equilibrium the constant Kp for the following reactions ( at 298.15K and 1bar). a. 2NO(g) +O2 (g) <----> 2 NO2(g) b. H2(g) + Cl2(g) <------> HCl(g) Based on the equilibrium constant, does the equilibrium favo the reactants or the products? TABLE molar Gibbs energies of formation, A Go, for various LU eJard substances at 29 K and one bar Substance Formula A Go /kJ.mol acetylene C2H2 209.20 ammonia NH3(g)...