The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.241 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K.

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.01420 mol of H2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4) = ______  .Peq(H2S) =  ______ .Peq(CS2) = ______  .Peq(H2) = _______  .(b) Calculate KP for this reaction.KP = _______  .

At a certain termperature, Kc = 0.914 for the reaction NO₂(g) + NO(g) = N₂O(g) + O₂(g) A mixture was prepared containing 0.200 mol NO2, 0.300 mol NO, 0.150 mol N₂O, and 0.250 mol O₂ in a 8.00 L container. What will be the equilibrium concentrations of each gas? [NO₂] [NO] [N₂O] [0₂] i i i i M M M M

5) At 25 °C the equilibrium constant of the reaction is Kel for the respective reactions and N₂(g) +3H₂(g) 2NH₂(g) (reaction 1) 3.5 x 108. What are the values Ke2 and Ke3 of the equilibrium constants = N2(g) +H₂(g) = NH₂(g) H₂(g) NH3(g), (reaction 2) 2NH3(9) N₂(g) + 3 H₂(g) 1 3 (reaction 3)?

The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g) is 26 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g) at 425 K?

Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g)2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 19.7 L container at 1150 K contains 0.251 mol of SO3(g) and 0.353 mol of SO2, the equilibrium concentration of O₂ is M. Submit Answer Retry Entire Group 9 more group attempts remaining

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.