Recall from our discussion of the NO,-N2O4 equilibrium that NO, has a brownish color. At elevated temperatures, NO2 reacts with CO according to NO2(g) + CO(g) 2 NO(g) + CO2(g) The other three gases taking part in this reaction are color- less. When a gas mixture is prepared at 500 K, in which 3.4 atm is the initial partial pressure of both NO, and CO, and 1.4 atm is the partial pressure of both NO and CO2, the brown color of the mixture is observed to fade as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).

Recall from our discussion of the NO,-N2O4 equilibrium that NO, has a brownish color. At elevated temperatures, NO2 reacts with CO according to NO2(g) + CO(g) 2 NO(g) + CO2(g) The other three gases taking part in this reaction are color- less. When a gas mixture is prepared at 500 K, in which 3.4 atm is the initial partial pressure of both NO, and CO, and 1.4 atm is the partial pressure of both NO and CO2, the brown color of the mixture is observed to fade as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A student ran the following reaction in the laboratory at 316 K:2CH2Cl2(g) CH4(g) + CCl4(g)When he introduced CH2Cl2(g) at a pressure of 0.487 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be 0.219 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 2 CH4(g) = C,H2(g) + 3 H2(g) K, = 1. × 10 He fills a reaction vessel at this temperature with 10. atm of methane gas. Use this data to answer the guestions in the table below. Can you predict the equilibrium pressure of C,H,, using only the О yes tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of C,H, at atm right. Round your answer to 1 significant digit.
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 1 atm of NOBr is sealed in a flask. At equilibrium, the partial pressure of NOBr is 0.82atm. What is the equilibrium constant, Kp, for the reaction?
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBR(g) =2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 298K contains NOBR at a pressure of 0.200 atm and NO at a pressure of 0.347 atm, the equilibrium partial pressure of Br2 is atm.
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) ⥂ 2 SO3 (g) At equilibrium, 0.0916 mol of SO3 is present. a.) What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b.) If the container size is 3.0 L, what is the value of the equilibrium constant?
Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)→CaCO3(s) At a certain temperature, a chemist finds that a 7.9 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount СаО 43.4 g CO2 19.6 g CaCO3 85.7 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = []
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 1.4 atm of sulfur dioxide gas and 1.2 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.3 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. db K = 0 x10 P X G
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 3.3 atm of sulfur dioxide gas and 3.2 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 2.6 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. K₁ = 0 P x10 X Ś
Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 5.0 L flask with 4.5 atm of ammonia gas and 4.5 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 2.0 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = | olo x10 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility .......................................
Consider the formation of phosgene: CO(g) + Cl₂(g) = COCl₂(g) Into a sealed 1.50 L flask, chemist placed 3.00 × 10-² mol of phosgene gas (COCl₂) and heated it to 800.0 K. After the system reached equilibrium, the pressure of CO was found to be 0.504 bar. Calculate the equilibrium constant Kp for this reaction. Calculate the initial pressure (in bar) of the phosgene gas. R = 0.08314 L.bar/mol K.