The system described by the reaction CO (g) + Cl₂ (g) = COC1₂ (g) is at equilibrium at a given temperature when Pco= 0.28 atm, Pa₂ = 0.12 atm, and PoocI₂ = 0.59 atm. An additional pressure of Cl₂ (g) = 0.42 atm is added. Part A Find the pressure of CO when the system returns to equilibrium. Express your answer using two significant figures. IVE ΑΣΦ P = 0.054 Submit Previous Answers Request Answer X Incorrect; Try Again atm

Suppose a 500. mL flask is filled with 1.3 mol of Cl₂ and 0.80 mol of HC1. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl (g) The equilibrium constant K for this reaction is 9.14 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś E A olo 18

What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s)   2 HI (g) + Cl2 (g)

Suppose a 500. mL flask is filled with 1.5 mol of H₂ and 1.2 mol of Cl₂. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 3.45 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M Ś

Consider the chemical reaction shown below with an equilibrium constant (K) of 3.0 at some temperature. You add 3.5 MA and 3.5 MB to a reaction vessel heated to this temperature. What will the reaction do to reach equilibrium? 2 A (g) 2 3 B (g) The reaction will form more reactants to reach equilibrium. O The reaction will form more products to reach equilibrium. O The answer depends on the volume of the reaction vessel. O Cannot be determined because the equilibrium constant changes over time. O The reaction is already at equilibrium.

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 50.0 L tank with 22. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 6.6 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = x10 X

For the reaction of nitrogen and oxygen to form nitrogen dioxide, N2(g) + 2 O2(g) → 2 NO2(g) Kc = 1.5×103 If the reaction mixture is found to contain 2.0 M NO2 and 0.10 M N2 and 0.10 M O2, what is the value of Q and what does this mean? is supposed to be an equilibrium arrow Q = 2x102 and the reaction will proceed towards the reactants. Q = 2x102 and the reaction will proceed towards the products. Q = 4x103 and the reaction will proceed towards the reactants. Q = 4x103 and the reaction will proceed towards the products.

A 25.0 g sample of nitrogen monoxide is injected into a 4.10–L reaction vessel that contains 13.8 g of nitrosyl bromide. When the system comes to equilibrium at 133 ℃, what is the total pressure inside the reaction vessel? The equilibrium constant, KC = 0.0863 at this temperature. R = 0.082058 L⋅atm/mol⋅K. Report your answer to THREE significant figures. 2 NO(g) + Br2(g) ⇌ 2 NOBr(g)

Suppose a 250. mL flask is filled with 1.4 mol of CO, 1.9 mol of H₂O and 1.0 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) 2 The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś ?

Consider the following reaction: N2 (g)  +  O2 (g) → 2 NO (g), Kc = 0.25 You start the reaction with 14.72 moles of NO (nitrogen monoxide) in a 2.0 L vessel. Calculate the concentration of O2 (in molarity) at equilibrium. (You do not need to solve a quadratic equation to solve this problem.)