Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂(g) S₂Cl₂(g) + CCL (g) Suppose 1.20 mol of CS₂ and 3.60 mol of Clą were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.23 mol CCl4. Calculate Ke at the unknown temperature. K.- Submit Answer Try Another Version References) 10 item attempts remaining

Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂(g) S₂Cl₂(g) + CCL (g) Suppose 1.20 mol of CS₂ and 3.60 mol of Clą were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.23 mol CCl4. Calculate Ke at the unknown temperature. K.- Submit Answer Try Another Version References) 10 item attempts remaining

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...

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ating UP bunE 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 liquld form It is easily transported. An Industrial chemist studying this reaction fills a 200. mL flask with 1.6 atm of ammonia gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.7 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 = Check Explanation 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility M 9 hp esc
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5L flask with 2.9 atm of carbon monoxide gas and 2.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.4 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.5 atm of carbon dioxide. The engineer then adds another 0.97 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 Submit Assignment Continue 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Air DII 888 F10 F8 F9 esc F6 F7 F4 F5 F3 F2 %23 $4 % - & 4. 5 8.
Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 1.64×10-3 moles of COCl2(g), 0.398 moles of CO, and 0.360 moles of Cl2 are at equilibrium in a 18.2 L container at 843 K, the value of the equilibrium constant, Kc, is .
Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Ch(g) =S,Cl½(g) + CC1,(g) When 1.14 mol of CS, and 4.80 mol of Clh are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.650 mol of CC14. How many moles of Cl are present at on equilibrium? Select one: O a. 0.490 mol O b. 2.85 mol O c. 3.50 mol O d. 0.650 mol O e. 1.43 mol e to search F3 F4 F5 F6 FZ FB F9 F10 F11 F12 Prise %24 E R T G H K B N M 立
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