What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 6.33e-8? 5C2H2(g) + 7 H2(g) ↔ C10H24(g) ΔGo = -908.030 kJ
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What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 6.33e-8?
5C2H2(g) + 7 H2(g) ↔ C10H24(g) ΔGo = -908.030 kJ
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- What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 4.56e-6?2C2H2(g) + H2(g) ↔ C4H6(g) ΔGo = -216.790 kJ. ΔGo = -219.346 kJ ΔGo = 589.938 kJ ΔGo = -214.234 kJ ΔGo = -247.262 kJWhat is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 5.95e-5?5C2H2(g) + 6 H2(g) → C10H22(g) ΔGo = -1.01e3 kJ. a) ΔG = -1.036e3 kJ b) ΔG = -1.010e3 kJ c) ΔG = -1.014e3 kJ d) ΔG = 1.057e3 kJCalculate the standard free energy, ΔGo, for the following equation at 25.0 oC and determine if the reaction is favorable or unfavorable. C2H6(g) + 7Cl2(g) ⟶ 2CCl4(g) + 6HCl(g) Group of answer choices 720.2 kJ/mole, unfavorable -656.2 kJ/mole, favorable 720.2 kJ/mole, favorable -720.2 kJ/mole, unfavorable 19.7 kJ/mole, favorable -656.2 kJ/mole, unfavorable 656.2 kJ/mole, favorable -19.7 kJ/mole, favorable -720.2 kJ/mole, favorable -19.7 kJ/mole, unfavorable 656.2 kJ/mole, unfavorable 19.7 kJ/mole, unfavorable
- 3. 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?Calculate the free energy change for the following reaction and predict whether the reaction occurs spontaneously at 25 °C and explain it. H2(g) + CO2(g) à H2O(g) + CO(g) ΔH = _____kJ, ΔS= ______J/KA spontaneous reaction always has: A. a positive enthalpy change and a negative entropy change. B. a positive Gibbs free energy change. C. a negative Gibbs free energy change. D. a standard enthalpy of formation equal to zero for one of the reactants. E. a standard free energy of formation equal to zero for one of the reactants.
- Calculate the standard free-energy changes for the following reactions at 25°C. a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) b. 2MgO(s) → 2Mg(s) + O2(g)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).What is the free energy change at 25°C for the reaction below, if ΔGfo(CH4(g)) = -50.790 kJ/mol, ΔGfo(C8H18(l)) is 7.584 kJ/mol.8CH4(g) ↔ C8H18(l) + 7H2(g)a) ΔGo = 58.374 kJb) ΔGo = 413.901 kJc) ΔGo = -58.374 kJd) ΔGo = -413.901 kJ
- The change of state from gaseous H2O to liquid H2O has a ΔH of -9.72 kcal/mol and a ΔS of -26.1 cal/(mol·K). What is the change in free energy of this reaction at 200K?Which of the following reactions corresponds to the reaction corresponding to a free energy of formation, ΔGfo? Group of answer choices.... 6 C(l) + 11 H2(g) + 11 O(g) → C6H22O11(s) P(g) + 4 H(g) + Br(g) → PH4Br(l) 6 C(s) + 6 H(g) → C6H6(l) 1/2 N2(g) + O2(g) → NO2(g) 2 N2(g) + 4 H2(g) + 3 O2(g) → 2 NH4NO3(s)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.