Determine the value of K c for the following reaction if the equilibrium concentrations are as follows: [HCl] eq = 0.13 M, [HI] eq = 5.6 × 10 -16 M, [Cl 2] eq = 0.0019 M.  2 HI( g) + Cl 2( g) ⇌ 2 HCl( g) + I 2( s)       3.5 × 10-32     1.4 × 10-19     8.2 × 10-18     2.8 × 1031     1.2 × 1017

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.

2A(g) ⇌ 1B (g) + 2C (g)                         ∆H ̊ = -69 kJ                K = 1 × 10-6   If the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium, the amount of B can be increased by: Group of answer choices Removing some A from the system Increasing the temperature of the reaction system Adding C to the system Increasing the volume of the reaction vessel

Write the equilibrium constant expression for the following reaction. Remember to use brackets, [ ], for concentrations and use exponents where needed, but do not show physical states in your answer.  C(s)  +  H2O(g)  ⇌  CO(g)  +  H2(g)   Keq =

4 Calculate the equilibrium constant, K, for the following: A + 2 B 3C +D when the equilibrium concentrations of each species were determined: [A] = 0.010 M, [B] = 0.15 M, [C] = 0.20 M, and [D] = 0.25 M.

For the reaction  2A(g) ⇌ 2B(g) + C(g),  Kc = 1.20 x10−7 at a given temperature.   If the initial concentration of A in a closed container is 0.610 M, what is the approximate equilibrium concentration of B?

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

What is the equilibrium concentration of HCL(g) if the initial concentration of H2(g) and Cl2 is 0.882 M. At that particular temperature, Kea=0.255 for the reaction: H2(g) + Cl2(g) 2 2HCI(g) 0.356 M O 0.704 O 0.298 M 0.882 M O 0.178 M

1. At a certain temperature, the value of K for the following reaction is 4.2 x 10. N₂(g) + O₂(g) → 2NO(g) 0.45 mol of nitrogen gas and 0.26 mol of oxygen gas are put in a 6.0 L reaction vessel. What is the equilibrium concentration of NO (g) at this temperature? Clearly show your steps