Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 50,(g) → 4 NO(g) + 6 H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,O 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 50,(g) → 4 NO(g) + 6 H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,O 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

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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Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N,(g) + 2 H,O(g) 2 NO(g) + 2 H,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 27.4 atm H,O 22.7 atm NO 51.8 atm H, 91.7 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = | Submit Assignmer Continue MacBook Air 80 F3 888 F4 F6 F2 $ % & 6 7 8 9
Hydrogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + O2(g) 2 Bг2(g) + 2 H₂O(g) - Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound pressure at equilibrium HBr 70.2 atm 0, 49.8 atm Br2 46.5 atm H₂O 75.7 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. = P x10
"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 2.0 L flask with 3.1 atm of carbon monoxide gas and 3.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.0 atm of carbon monoxide gas, 1.5 atm of water vapor and 2.1 atm of carbon dioxide. The engineer then adds another 0.90 atm of water, 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. 0 atm x10 C [
Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10
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Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) 2 NO(g) + 2 H2(g) → Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 92.2 atm H,O 76.1 atm NO 19.3 atm H2 33.6 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0
Nitrogen and hydrogen react to form ammonia, like this: N,(g) + 3 H,(g) → 2 NH,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N2 82.3 atm H2 38.7 atm NH3 73.0 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
"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.
Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br, (g) + 2 H,0(g) - 4 HBr(g) + 0,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition: compound pressure at equilibrium Br, 49.2 atm H,0 80.9 atm HBr 94.3 atm O2 62.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. * = 0
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Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.
Nitrogen monoxide and water react to form ammonla and oxygen, Ilke this: 4 NO(g) + 6H,O() 4 NH,(g) + 50,(g) Also, a chemist finds that at a certain temperature the equilibrlum mixture of nitrogen monoxide, water, ammonia, and oxygen has the followng composition: compound pressure at equilibrium NO 12.7 atm H,0 94.3 atm NH3 58.1 atm 0, 93.8 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. d. K = x10 Check Explanation ©2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Ac M9 hp & esc % * 00 96 %24