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Determine AGⓇ for a reaction at 298 Kelvin, If the equilibrium constant is 7.38 x 102?...
Determine the equilibrium constant for the following reaction at 298 K: SO3(g) + H2O(g) → H2SO4(l) ΔG°rxn = -90.5 kJ mol-1 Group of answer choices 0.964 4.78 × 1011 7.31 × 1015 1.37 × 10-16 9.11 × 10-8
How would the equilibrium constant change if the reaction X with AGⓇ = +12.2 kJ moll was coupled to the hydrolysis of ATP (AGⓇ' = -30.5 kJ mol-!)? Consider that R* T is equal to 2.47. would increase by a factor of 105 would increase by a factor of 106 would decrease by 5.15 would increase by 5.15 would decrease by a factor of 106
Determine AGⓇ for a reaction when AG = -184.7 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol K)
20. What is AS at 298 K for the following reaction? CH4(g) + N2(g) → HCN(g) + NH3(g); AH = 164.1 kJ; AGⓇ = 159.1 kJ at 298 K a. 17 J/K b.5.5 x 102 J/K c. 5.3 x 102J/K d. 1.1 x 10 J/K e. 2.0 J/K 21. Given the following, determine 208 Kunne male
() Calculate AGⓇ for the following reaction at 298 K. The AGP values are 0 kJ/mol for C12(e) -325 kJ/mol for Cisce), and -286 kJ/mol for PC13(e). PC1518) PC3(8) + Cl2(g) (b) Calculate AG at 298 K for the reaction if the partial pressures are PC120,40 atm, PPC13 -0.27 atm, and PPCi5 -0.0029 atm.
A reaction has an equilibrium constant of 8.4 x 10^3 at 298 K. At 800 K, the equilibrium constant is 0.72. Find ∆H°rxn for the reaction. (in kJ)
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(a) Calculate AGⓇ for the following reaction at 298 K. The AGP values are 0 kJ/mol for Cl2(e) -325 kJ/mol for PC (e), and -286 kJ/mol for PC13(e). PCIE) - PC3(g) + Cl2(8) (6) Calculate AG at 298 K for the reaction if the partial pressures are PC12 -0.40 atm, PPC13 - 0.27 atm, and PPCIS -0.0029 atm.
A first-order reaction has a rate constant of 1.35 x 102 s-1 at 25.0 oC (298 K). The energy of activation is 55.5 kJ mol-1; and the frequency factor is 7.23 x 1011 s-1. What is the value of the rate constant (k) at 95.0 oC (368 K)?
Determine the equilibrium constant at 298 K for the reaction: Zn (s) + Ni2+ (aq) Zn2+ (aq) + Ni (s) (Hint: Start with the E°) A) (4.1 ± 0.1) x 10 3 B) (1.7 ± 0.1) x 10 17 C) (9.3 ± 0.1) x 10 8 D) (6.4 ± 0.1) x 10 -6 --------------------------------------------------------------------------------------------------------------- Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g). Assume ΔH°rxn = 41.0 kJ/mol for all temperatures in this problem. If Kp = 5.10 at...
A reaction has an equilibrium constant of 8x103 at 298 K. At 716 K, the equilibrium constant is 0.77. Find AHºrxn for the reaction. Enter your answer numerically in kJ to 4 decimal places.