The Kp for th reaction 2 A2B(g)⇌ 2 A(g)+B2 (g) is 2.2*10^-5. The gas is introduced to the reaction vessel of a fixed volume at the partial pressure of 0.010 atm. Explain how you would  find the total pressure at equilibrium. The systems temperature is the same for the Kp value and stays constant for the entire reaction. You do not have to solve for the actual pressure, but explain what would be used to do so.

Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.110 M and [12] = 0.270 M. The equilibrium constant Kc for the reaction H2(g) +I2(g) = 2 HI(g) is 57.0 at 700 K. Part A Calculate the equilibrium concentrations of H2. Express your answer to three decimal places and include the appropriate units.

Indicate the major organic product from the reaction shown. CuLi Br

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: (3)H+(3)0ɔ= (3)0°H+(3)0) The equilibrium constant K for this reaction is 0.735 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. OM

Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)

Assume that the change in concentration of COCl2 is small enough to be neglected in the following problem. Use an ICE table with the "x is small" approximation. The results might surprise you. You can trust them if you verify the assumption. (a) Calculate the equilibrium concentration of all species in an equilibrium mixture that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g) + Cl2(g)       Kc=2.200 × 10−10 Enter the equilibrium molar concentration of COCl2 below, with 4 sig figs

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g)     A )Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms.    Qc = _____/_____ = _____   Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.          Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴   Based on your ICE table and expression for Kc, solve for the concentration of O₂ at equilibrium. [O₂]eq = _____M

The equilibrium constant, Kc, for the following reaction is 1.20\times 10 - 2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.331 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.