As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (a) and 0.750 mol N204 (g) at 25°C. Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N204 (g) → 2NO2 (g) K = 4.61 x 10-3 at 25°C

For the reaction: 2CO2 (g) = 2CO(g) + O₂(g), What can be said about this reaction at this temperature? K = 1.00 × 10-13 at 1200 K The equilibrium lies far to the left. The reaction goes to completion. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the right.

Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.50 mol of H₂O and 1.2 mol of CO₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂(g) +H₂(g) The equilibrium constant K for this reaction is 0.503 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M ܢܢ X E 00 Ar

At 30 degrees Celsius the Kc for 2CO(g) + O2(g) = 2CO2(g) is 2.24 x 1022. Predict in which direction the reaction will proceed to reach equilibrium, if we start with 55.0 g CO, 95.0 g O2 and 75.0 g CO2 in a 5.0 L vessel.

Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H₂, 8.0 M N₂, and 4.0 M NH 3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. N₂(g) + 3 H₂(g) = 2 NH3(g) Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2.0 0 2.0 5.0 -5.0 N₂(g) 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) -4.0 10.0 2 NH3(g) RESET 11.0

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×

Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas

Consider the reaction;  N2(g) + O2(g)⇆ 2 NO(g)  where K = 0.10.      Starting with initial concentrations of [N2] = 0.04 M and [O2] = 0.40 M,      the equilibrium concentration of NO is

Which of the following equilibrium expressions (K) represent the equilibrium reaction: 2 Fe(s) + 3 Cl2(g) = 2 FeCl3(s)