PCl5 (g) ⇌ PCl3 (g) + Cl2 (g) Initially, 0.798 M PCl5 is placed in a reaction vessel and the reaction is allowed to reach equilibrium. If the equilibrium constant for this reaction is 6.58 M, what is the equilibrium concentration of PCl5 in M?

The equilibrium constant, K, for the following reaction is 1.80×10-² at 698 K. 2HI(g) H₂(g) + I₂(g) If an equilibrium mixture of the three gases in a 19.0 L container at 698 K contains 0.230 mol of HI(g) and 0.345 mol of H₂, the equilibrium concentration of 12 is M.

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g)   1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms   2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.   3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown.   4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.

Suppose a 500. mL flask is filled with 1.8 mol of Cl,, 1.6 mol of CHCI, and 1.7 mol of HCl. The following reaction becomes possible: Cl,(g) +CHCI, (g) HCl(g)+CCl,(g) The equilibrium constant K for this reaction is 0.642 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places.