Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BIOC1 and 1.6 mol of BrCl. The following reaction becomes possible: Br, (2)+OC1,(2) - BIOCI(2) + BICI(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BIOC1 and 1.6 mol of BrCl. The following reaction becomes possible: Br, (2)+OC1,(2) - BIOCI(2) + BICI(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.

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

The equilibrium constant, K., for the following reaction is 9.52x102 at 350 K. CH4 (g) + CC14 (g) = 2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.251 moles of CH4 and 0.251 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CCI4 ] [ CH,Cl, ] = | M M M
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.
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
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 1.9 atm of methane gas and 2.1 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.6 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
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -2 N2(g) + 3 H,(g) 2 NH3(g) K,=4. x 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.5 atm of hydrogen gas. Use this data to answer the questions in the table below. dla O yes Can you predict the equilibrium pressure of NH, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NH, at right. ||atm Round your answer to 1 significant digit. Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Accessibility
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 5.0 L flask with 0.93 atm of methane gas and 2.7 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 0.47 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_ = || x10
The equilibrium constant, K, for the following reaction is 6.30 at 723 K. 2NH3(g) ⇒N₂(g) + 3H₂(g) If an equilibrium mixture of the three gases in a 10.9 L container at 723 K contains 0.409 mol of NH3(g) and 0.291 mol of N₂, the equilibrium concentration of H₂ is M.
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 1.5 L flask with 3.2 atm of methane gas and 1.1 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 2.0 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, = I
Suppose a 500. mL flask is filled with 0.20 mol of Br,, 1.6 mol of OCl, and 1.9 mol of BrOCl. The following reaction becomes possible: 2' Br, (g) +OCl, (g)- BROCI(g)+BrC1(g) The equilibrium constantK for this reaction is 5.57 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. O M
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)
Suppose a 500. ml. flask is filled with 0.60 mol of Br₂, 0.70 mol of BrOCI and 0.20 mol of BrCl. The following reaction becomes possible: Br₂(g) +OCI, (8) BrOCI(g) + BrCI(g) The equilibrium constant K for this reaction is 7.17 at the temperature of the flask Calculate the equilibrium molarity of OCI, Round your answer to two decimal places. M
O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II