Consider the following system at equilibrium at 698K: 2HI(g) + 2.49 kcal ->H2(g) + I2(g)  If the temperature on the equilibrium system is suddenly decreased: The reaction must: ____  The concentration of I2 will ____

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is

Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.

Can you please answer question 2

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 5.40x10-4 moles of NH3(g), 0.450 moles of N₂, and 0.215 moles of H₂ are at equilibrium in a 15.1 L container at 846 K, the value of the equilibrium constant, K, is

Help with the following question Please round the answer to 2 decimal places