At a certain temperature, 0.3811 mol of N₂ and 1.761 mol of H₂ are placed in a 4.50 L container according to the following equation: N₂(g) + 3H₂(g) + 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.

Suppose a 500. mL flask is filled with 1.8 mol of CO, 1.9 mol of H,0 and 1.6 mol of H,. The following reaction becomes possible: co (g) +H,0(g)– CO,(g) +H2 (g) The equilibrium constant K for this reaction is 0.275 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 1.5 mol of H₂O, 0.10 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.980 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X

Suppose a 250. mL flask is filled with 0.90 mol of Cl₂, 1.2 mol of HCl and 2.0 mol of CC14. The following reaction becomes possible: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) The equilibrium constant K for this reaction is 0.702 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places.

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

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 50.0 L tank with 4.7 mol of sulfur dioxide gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 3.3 mol, Calculate the concentration 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 X

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For the chemical equation so, (g) + NO, (g) SO, (g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.31 mol SO, (g) in order to form 1.10 mol SO, (g) at equilibrium. moles of NO, (g): mol

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 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 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

Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOC1 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 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. ?