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- Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.At 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction? C₂H₄ (g) + H₂ (g) → C₂H₆ (g)
- Calculate Hrxn for the reaction below. CO(g) + NO(g) CO2(g) +1/2 N2(g) You are given the following set of reactions. CO(g) + 1/2 O2(g) CO2(g) H = -283.0 kJN2(g) + O2(g) 2 NO(g) H = 180.6 kJA potential chemical reaction at 25.0 °C has a ΔHrxn of 163 kJ and a ΔSrxn of -354.3 J/K. What is the ΔGrxn in kJ.Calculatre the ΔH of reaction for the following reaction: Fe3O4 (s) + CO (g) --> 3FeO (s) + CO2 (g) ΔHfo (kJ/mol) -1118 -110.5 -272 -393.5 a -263 kJ b 54 kJ c 19 kJ d -50 kJ e 109 kJ
- Calculate Kp at 25 °C for the following reaction: 2 H2 (g) + O2 (g) ⇋⇋ 2 H2O (g) Kc = 3.2 x 1081 at 25 °C Round your answer to 2 significant figures.Calculate the value of K for the formation of NO2 from NO and O2 at 298 K if ∆?° = -35.3 kJ/ mol for the following reaction. (R = 8.314 J/mol. K) NO(g) + 12 O2 (g) ⇌ NO2 (g)What is ∆G° for the reaction Br₂(g) → 2 Br(g) at 25.0 °C if K = 4.6 x 10⁻²⁹? (R = 8.314 J/mol･K) in kJ/mol
- What is ∆G° for the reaction CH₃OH(g) → CO(g) + 2 H₂(g) at 25°C?The value of Keq for the following reaction is 0.16: A (g) + B (g) <==> C (g) + D (g) The value of Keq at the same temperature for the reaction below is ________. 3C (g) + 3D (g) <==> 3A (g) + 3B (g) A) 2.4 × 102 B) 2.1 C) 4.1 x 10-3 D) 5.3 x 10-2 E) 6.3What must the reaction quotient Q be, if the free energy is -961.941 kJ at 25.0°C? 5C2H2(g) + 5 H2(g) → C10H20(g) AGO = -925. 150 kJ.