50.0 g of N2O4 is introduced into an evacuated 2.00 L vessel and allowed to come to equilibrium with its decomposition product, N2O4(g) ⇌ 2NO2(g). For this reaction Kc = 0.133. Once the system has reached equilibrium, 5.00 g of NO2 is injected into the vessel, and the system is allowed to equilibrate once again. Calculate the mass of N2O4 in the final equilibrium mixture.

Phosphorus pentachloride decomposes according to the chemical equation. PCI5 (g) PCI 3 (g) + Cl 2 ( g) Kc = 1.80 at 25 0 C. A 0. 3200 mol sample of PCI 5 (g) is injected into an empty 3.8 L reaction vessel held at 2 5 0 C. Calculate the concentrations of PCI 5 (g ) and PC| 3 (g) at equilibrium.

For the reaction N₂O₄(g) ⇌ 2NO₂(g) Kc = 4.66 × 10⁻³ at 25°C . 2.50 g N₂O₄ and 0.250 g NO₂ are introduced into a 2.00-L reaction vessel. After equilibrium is achieved, what is the concentration of NO₂?

For the reaction N₂O4(g) = 2NO₂(g) Kc = 4.66 x 10-³ at 25 °C. 2.50 g N₂O4 and 0.440 g NO₂ are introduced into a 2.00-L reaction vessel. After equilibrium is achieved, what is the concentration of NO₂?

For the reaction N₂O₄(g) ⇌ 2NO₂(g) Kc = 4.66 × 10⁻³ at 25 °C . 2.50 g N₂O₄ and 0.370 g NO₂ are introduced into a 2.00-L reaction vessel. After equilibrium is achieved, what is the concentration of NO₂?

A mixture containing 5.6 Atm of N2O and 2.8 Atm of O2 was prepared and after the equilibrium                         2 N2O(g) + 3 O2(g)  ⇆  4 NO2(g) was established the O2 partial pressure was found to be 0.31 Atm. What is the equilibrium constant Kp?

Consider the following reaction and its equilibrium constant: 12 (g) + Br2 (g) ÷ 2 IBr (g) Kc = 1.1 × 102 A reaction mixture contains 0.41 M I2, 0.27 M Br2 and 2.2 M IBr. Which of the following statements is TRUE concerning this system? O The equilibrium constant needs to increase. The reaction needs to shift in the direction of the reactants to reach equilibrium. O The system is at equilibrium. O The reaction needs to shift in the direction of the products to reach equilibrium.

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

For the reaction: 2CO2 (g) = 2CO(g) + O₂(g), What can be said about this reaction at this temperature? K = 1.00 × 10-13 at 1200 K The equilibrium lies far to the left. The reaction goes to completion. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the right.

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of sulfur dioxide gas and 0.67 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.80 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P 0 x10