Consider the endothermic reaction below, which is at equilibrium in a 2 L container. A (g)  +  2Z (g)  ⇌  AZ2 (g) If the temperature is increased, the concentration of AZ2 will (increase, decrease, or remain the same).  If the volume of the container is decreased to 1 L, the reaction will (shift left or shift right) to reestablish equilibrium. If reactant A is removed from the reaction vessel, the concentration of AZ2 will (increase, decrease, or remain the same).

Determine whether the system below is in equilibrium or not: Write the equilibrium expression of the reaction above. If the system is not in equilibrium, predict whether it will proceed in the forward or reverse direction H2 (g) + I2 (g) = 2HI [H2] = 0.10M; [I2] = 0.10M; [HI] = 0.70M; Keq = 49

NAME: COC12(g) has a 8. At 100.0°C, the equilibrium constant for the reaction: COg) + Cl2(g) value of 4.6 x 10°, If 0.40 mol of COC12 is placed into a 10.0 L flask at 100.0°C, what will be the equilibrium concentration of all species? (A simplifying approximation that will make the solution of the resulting equation easier is to note that X is much less than 0.040 mol/L. This means that 0.040-x is approximately 0.040.)

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

For the reaction 2 NO(g) + Cl2 (g) *double arrow here* 2 NOCl (g) at 25 ℃, the equilibrium constant is 10.0. If at equilibrium, [NOCl] = 2.6 M, [NO] = 0.34 M, what is the concentration of chlorine gas?

Assume that the following exothermic chemical reaction is at equilibrium. CuO (s) + H2 (g) ⇌ H2O (g) + Cu (s). Which of the following statements is CORRECT? Choose one option. a. Increasing the concentration of H2 (g) will cause the reaction to proceed in the backward direction (shift to left), increasing the equilibrium concentration of H2O (g). b. Decreasing the temperature will cause the reaction to proceed in the forward direction (shift to right), increasing the equilibrium concentration of H2O (g). c. Increasing the amount of CuO(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of H2O (g). d. Increasing the temperature will cause the reaction to proceed in the forward direction (shift to right), increasing the value of the equilibrium constant of this reaction. e. The value of the equilibrium constant for this reaction will stay the same after the temperature is increased.

Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]

N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)

A 1.0 L flask is filled with NO and O2 initially, and, after the reaction establishes equilibrium, the flask is found to contain 0.0018 mol NO, 0.0012 mol O2 and 0.78 mol NO2. What is the value of the equilibrium constant, Kc, at this temperature? 2 NO(g) + O2(g) → 2 NO2(g) is supposed to be an equilibrium arrow 6.3x10-9 2.8 x 10-6 3.6 x 105 1.6 x 108