For the equilibrium:                     2 BrCl (g)   à   Br2 (g) + Cl2 (g) at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.58 moles each of Br2 (g) and Cl2 (g) are introduced in a container which has a volume of 15.3 liters and allowed to reach equilibrium at 205 °C, what would be the concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium?

Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?

At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.400 mol H2 and 0.400 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI]= M   At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.13×10−3. At equilibrium, the concentration of AB is 2.725 M, the concentration of BC is 2.225 M, and the concentration of AC is 0.220 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) [B]= M

For the equilibrium: 2 BrCl (g) --> Br2 (g) + Cl2 (g) at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.34 moles each of Br2 (g) and Cl2 (g) are introduced in a container which has a volume of 11.0 liters and allowed to reach equilibrium at 205 °C, what would be the concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium?

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 1.1: Cl₂(g) + CHCl3(g) → HCl(g) + CCl4(g) Use this information to complete the following table. Suppose a 8.0 L reaction vessel is filled with 0.35 mol of HCI and 0.35 mol of CCl4. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. HCl(g)+CC1,(9) Cl₂(9)+CHC13 (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 3 Cl₂(g) + 3 CHCl3(g) P 3 HCl(g)+3CCI (9) There will be very little Cl₂ and CHCl3. There will be very little HCI and CCI4. Neither of the above is true. K = 0 K = 0 x10 X 5 olo 18 Ar U

Phosphorus pentachloride decomposes according to the chemical equation Ke = 1.80 at 250 °C PC15 (g) ⇒ PC13(g) + Cl₂(g) A 0.3606 mol sample of PC15 (g) is injected into an empty 3.95 L reaction vessel held at 250 °C. Calculate the concentrations of PC15 (g) and PC13 (g) at equilibrium. [PCI,] = [PC1₂] = M M

Calculating an equilibrium constant from a partial equilibrium composition Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 1.5 L flask with 4.3 atm of methane gas and 1.8 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.2 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K p 11] ☐ x10 ☑ ⑤

A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр

Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?

At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.