1a) Consider the following reaction:
3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ; ΔS° = –287.4 J/K at 298 K
What is the equilibrium constant at 298 K for this reaction? Report answer to TWO significant figures.
1b) Τhe enthalpy of vaporization of ammonia is 23.35 kJ/mol at its boiling point (–33 °C). Calculate the value of ΔSsurr when 1.00 mole of ammonia is vaporized at –33 °C and 1.00 atm. Report answer to THREE significant figures.
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1a) Consider the following reaction: 3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ;...
1) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(g); AH° = -104.7 kJ; AS = -287.4J/K at 298 K What is the equilibrium constant at 300.0 K for this reaction? AGº = -RT In K. AG° = AH° - TAS" (R=8.3145J/mol.K) (6 points)
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
Question 29 (9 points) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(8); AH° =-104.7 kJ; ASP = -287.4J/K at 298 K 1). What is AGⓇ for this reaction? 2). What is the equilibrium constant at 400.0 K for this reaction?
For the reaction: C(s) + H2O(g) CO(g) + H2(g), ΔH° = 131 kJ and ΔS° = 128 J/K at 298 K. At temperatures greater than ______ K, this reaction is spontaneous under standard conditions. a. 1.02 K b. 273 K c. 1023 K d. 753 K
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.
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.
Question 12: (1 point) What are the values of q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following a constant pressure process for a system containing 0.572 moles of CH3OH ? CH3OH(l, 26.0 ºC, 1.00 atm) ⟶ CH3OH(g, 118.0 ºC, 1.00 atm) Assume that the volume of CH3OH(l) is much less than that of CH3OH(g) and that CH3OH(g) behaves as an ideal gas. Also, assume that the temperature of the surroundings is 118.0 ºC. Data: Molar heat capacity for CH3OH(l), Cp,m...
Consider the following reaction: 2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K Assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 34 ∘C. Express your answer using four significant figures.
Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy of vaporization ( Δ S^ovap) = 36.1 J/K mol. Calculate the boiling point of liquid nitrogen, in oC using this information. (Use 273.15 K = 0 oC for the temperature conversion. Report your answer with three significant figures.) Tvap = ????? °C I got 196^oC but it is incorrect.
Consider the following reaction at 298 K.C(graphite) + 2H2(g)→ CH4(g) ΔH°=-74.6 kJ