3 Ni(s) + N₂(g) + 3 H₂O(g) 3 NIO(s) + 2NH3(g) where K = 6.74 x 10-4 At what partial pressure of ammonia will one be able to get out 11.5 kJ/mol of Gibbs free energy from this reaction when the rest of the mixture contains 57.6 g NiO, 182.3 g Ni, 8.54 atm of nitrogen gas, and 10.07 atm of water vapor? | atm

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 104. kJ. Calculate the temperature at which the equilibrium constant K = 7.1 × 10¹8. Round your answer to the nearest degree. T = °C X S

For the equation:   CH3OH (l) + 3/2 O2(g) -> CO2 (g) +2H2O   What drives this reaction to go in the forward direction? Entropy, Enthropy, both, or neither?

For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature

For a certain chemical reaction, the standard Gibbs free energy of reaction at 20.0 °C is 90.2 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = || x10

You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in Gibbs free energy (∆G) for this process?

Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) AGixn || - 2 HNO3 (1) + NO(g) kJ/mol

Consider the following rection:             2 A(g) + B2(g) ⇌  2 AB(s)            If Kc for the reaction is 0.271 and ΔH° for the reaction is 5.17 kJ at 493.6 What is the value of Kc at 1,162.1 oC ? (R=8.314 j/molK) Report your answer with three decimal. Enter numbers only; do not enter units.