The equilibrium constant for the reaction shown below is 61.2 H, (g) + Br, (g) = 2HB1(g) Write an expression for the equilibrium constant, K What is the equilibrium concentration of Br2, if [HBr]=0.48 M and [H2] = 0.26 M at equilibrium?

Suppose a 250. mL flask is filled with 1.2 mol of NO and 0.90 mol of NO 2. The following reaction becomes possible: NO3(g) + NO(g) = 2NO2(g) The equilibrium constant K for this reaction is 0.661 at the temperature of the flask. Calculate the equilibrium molarity of NO 3. Round your answer to two decimal places. Ом ☑

Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐M X 5

Consider the reaction: 2 CO(g) + O₂(g) 2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

My question is below. Any help would be appreciated. Consider the following reaction: CO (g) + 2 H2 (g) = CH3OH (g) A reaction mixture in a 5.15 L flask at a certain temperature initially contains 27.1 g CO and 2.32 g H2. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature.

Consider the decomposition reaction: X(g) + 2 Y(g) XY2(s) where X and Y are some chemical groups. At a certain temperature the equilibrium constant for this reaction is Ke= 0.108. If you start with a large amount of XY2 (s), c= what will be the concentration of Y(g) once the system reaches equilibrium? (HINT: Draw an ICE table or you will likely get this wrong!) (A) 0.108 M (B) 0.216 M (C) 0.300 M (D) 0.600 M (E) 1.08 M

Suppose a 250. mL flask is filled with 0.80 mol of O2 and 0.30 mol of SO3. This reaction becomes possible: 2SO2(g) + O2(g) ~ 2SO3(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use r to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity.

Suppose a 500. mL flask is filled with 1.9 mol of N, and 0.20 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 3.27 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.8 mol of O2 and 0.30 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 2.61 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. M X S

Suppose a 500. mL flask is filled with 1.1 mol of NO2, 1.7 mol of NO and 0.90 mol of CO2. The following reaction becomes possible: NO, (g)+CO(g) NO(g) +CO,(s) The equilibrium constant K for this reaction is 0.292 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. м B C ol