3. For the following system at equilibrium N2(g) + 3H₂(g) 2 NH3(g) K = 626 at 200°C the equilibrium concentrations of hydrogen and ammonia are 0.50 mol/L and 0,46 mol/L, respectively. Calculate the equilibrium concentration of nitrogen.

Suppose a 500. mL flask is filled with 1.7 mol of Br,, 1.4 mol of OCl, and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g)- BROC1(g)+BrC1(g) The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. olo ? Ar G Explanation Check © 2022 McGraw Hill LLC. AIL Rights Reserved. Terms of Use | Privacy Center | Accessibility

At a particular temperature 8.0 mol NO2 gas is placed in a 1.0-L container. Over time the NO2 decomposes to NO and O2: 2NO2(g) 2 2NO(g) + O2(g) At equilibrium the concentration of NO(g) was found to be 1.8 mol/L. Calculate the value of K for this reaction (using units of mol/L for the concentrations). K =

Steam reforming of methane ( CH ) 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 25.0 L tank with 7.0 mol of methane gas and 1.8 mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 1.4 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = || %3D Submit Assignn

1. At 100 C the equilibrium constant, Kc is 4.6 x 10° for the reaction, CO (g) + Cl₂ (g) = COC1₂ (g). If 0.20 moles of COCl2 is placed in a 10.0 liter container, what is the concentration of all species at equilibrium?

Consider the reaction: 2 CO(g) + O₂(g) 2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

the equilibrium constant K for the following reaction is 6.35 x 10: 2 HCl(g) At a certain temperature, H₂(g) + Cl₂(g) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.3 mol of H₂ and 1.3 mol of Cl₂. 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 3 significant digits. 2 HC1(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 H₂(g) + 3Cl₂(g) 6 HCl(g) There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0

Steam reforming of methane ( CH, ) 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 2.0 L flask with 3.8 atm of methane gas and 2.0 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.0 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, 0 x10 ?

Calculating equilibrium composition from an equilibrium constant Suppose a 250, mil. flask is filled with 1.5 mol of NO₂, 0.10 mol of CO and 2.0 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.226 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. OM Explanation CIU Check DEC 9 X 3 6 tv 8

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 500. mL flask with 1.2 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.60 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 x10 5