Calculate the equilibrium constant, K, of a reaction that occurs at 25°C.  This reaction has a free energy change, ΔG°, equal to -52.3 kJ/mol.  Group of answer choices A, 2.69e-5 B, 2.35e5 C, 1.47e9 D, 4.99e-6

A2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium? b) What is the value of ΔGrxn assuming the temperature is maintained at 25oC?

Calculate A,G° at 25 °C for the formation of 1.00 mol of C2H5 OH(g) from C2H4(g) and H20(g). Use this value to calculate K, for the equilibrium. C2H4 (g) + H2O(g) 2 C,H;OH(g) Use the following data: kJ A;G*, mol C2H4 (g) H2O(g) C2H; OH(g) 68.35 -228.59 -168.49 Kp The v value of A,G' and the v value of Kp indicate that the reaction is product-favored.

Determine AG° for the reaction 2 SO,(g) + 0,(g) →2 SO3(g) at 25 °C. Thermodynamic Data at 25 °C Species AH? in kJ/mol AG? in kJ/mol S° in J/(mol·K) O2 (g) SO2 (g) SO3 (g) 0. 205.0 -296.8 -300.1 248.2 -395.7 -371.1 256.8

[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = -111 kJ/mol, and K. = 0.159 , at 723 K. N2 (g) + 3 H, (g)=2 NH3 (g) When 0.21 moles of NH, (g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish coquilibrium. O remain the same. It is already at cquilibrium. The concentration of H, will Submit Answer Retry Entire Group 1 more group attempt remaining

For the reaction 2HBr(g) + Cl₂ (g) → 2HCl(g) + Br₂ (g) AH = -81.1 kJ and AS° = -1.20 J/K The equilibrium constant for this reaction at 288.0 K is | Assume that ΔΗ° and AS are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining

Calculate the temperature at which the reaction below will be at equilibrium, then explain how this temperature can affect the spontaneity, meaning how using higher or lower than this temp can affect the value of delta G.   Given.      Br2(l) → Br2 (g),  ΔH = 31.0 kj/mol ΔS = 92.9 j/mol