Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g) →3 NO,(9)+H,O(1) At a certain temperature, a chemist finds that a 8.4 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 14.7 g NO 21.2 g NO, 21.4 g H,0 129.9 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = |

Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g) →3 NO,(9)+H,O(1) At a certain temperature, a chemist finds that a 8.4 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 14.7 g NO 21.2 g NO, 21.4 g H,0 129.9 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = |

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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A container with a volume of 1.70 L was evacuated and then filled at low temperature with 0.0370 mol liquid dinitrogen tetroxide, N204. As the temperature was raised, this substance formed nitrogen dioxide, NO2 : N204(9) = 2NO2(g) a If the pressure of this reaction mixture at equilibrium at 25.0°C was 0.656 atm, what was the total moles of gas in this mixture? mol
Methanol and oxygen react to form carbon dioxide and water, like this: 2 CH;OH(1)+3 O,(g)→2CO,(g)+4 H,0(g) At a certain temperature, a chemist finds that a 2.6 L reaction vessel containing a mixture of methanol, oxygen, carbon dioxide, and water at equilibrium the following composition: compound amount CH,OH 1.64 g 1.70 g Co, 2.46 g H,0 2.47 g Calculate the value of the equilibrium constant K. for this reaction, Round your answer to 2 significant digits. K. - ] Fxplanation Check anes Beserved Tom of Use P Type here to search ZI Alt Alt Ctrl Home
Calculating an equilibrium constant from a heterogeneous... Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO,(aq)+NO(g)-3 NO,(g)+H,0(I) At a certain temperature, a chemist finds that a 6.1 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 8.2 g NO 24.9 g NO, 12.7 g H,0 76.7 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = ]
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g)→3 NO,(9)+H,0(1) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 16.7 g NO 17.8 g NO, 8.7 g H,0 208.3 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0
Suppose a 500. mL flask is filled with 1.9 mol of O, and 1.8 mol of SO2. This reaction becomes possible: 2s0,(g) +0,(g) – 2so,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. So, O2 initial 口 D. change equilibrium
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Suppose a 500. mL flask is filled with 1.3 mol of NO and 0.90 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g) — 2NO₂(g) The equilibrium constant K for this reaction is 0.720 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X Ś
E8hstant from a heterogeneous. Iron(III) oxide and hydrogen react to form iron and water, Ilike this: Fe,0;(s)+3 H,(9)→2 Fe(s)+3H,O(g) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has following composition: compound amount Fe,O3 4.85 g H2 2.01 g Fe 3.53 g H,O 1.33 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = | Explanation Check 2022 McGraw H LLC A Rights Reservedt Tem of Use acy Conter Accesbity Type here to search 99 C FIO Pr Sc 24 4. & he 7. 8. %3D Y U H K Alt Alt Chl
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Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO,(aq)+NO(9)-3 NO,(g)+H,0(1) At a certain temperature, a chemist finds that a 5.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 22.6 g NO 15.5 g NO2 21.9 g H,0 107.8 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K, = 0 Plecy Terms of Use ©2021 McGraw-Hl Education All Rights Reserved Check Explanation
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₂=6. × 10 -8 He fills a reaction vessel at this temperature with 7.0 atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. 0 yes no atm x10 X Ś
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