For the following reaction, N₂O(g) + ¹/2 O₂(g) = 2 NO(g) Calculate the equilibrium constant at 298 K AG° = 68.9 kJ/mol at 298 K. A. 8.4 x 10-13 B. 0.97 C 28

8.B A certain reaction has an equilibrium constant of K = 8.3×10$ at 25°C with a temperature-independent standard enthalpy of reaction of 34.2 kJ/mol. (a) What is the equilibrium constant at 37°C? (b) Use Le Chatelier's principle to defend your answer.

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

Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D

What is AG for the reaction l2(g) → 2 1(g) at 25.0 °C if K = 6.1 x 10-2²? (R = 8.314 J/mol.K)

At 460 K, AG = -10.8 kJ/mol for the reaction 2 A (g) → B (g). If the partial pressures of A and B are 7.20 atm and 0.420 atm respectively, what is AG° for this reaction? kJ/mol 1 6. C 8. 6. R +/- x 100 nic ribe 4.

Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NH3(g) →>> 4 N₂H₁(g) + H2(g) Round your answer to 2 significant digits. K = П ☐ x10 ☑ 0/5 izabella ? ola 18 Ar 館