Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO,(9)+H2O(1)→2 HNO3(aq)+NO(9) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO, 24.5 g H,O 67.1 g HNO3 7.8 g NO 9.2 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K. %D

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO,(9)+H2O(1)→2 HNO3(aq)+NO(9) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO, 24.5 g H,O 67.1 g HNO3 7.8 g NO 9.2 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K. %D

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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Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐M X 5
Suppose a 250. mL flask is filled with 0.90 mol of N, and 1.2 mol of NH2. This reaction becomes possible: ME N,(g) +3H,(g) – 2NH, (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 N,. You can leave out the M symbol for molarity. H, NH, initial change equilibrium Continue Submit As O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center 43,203 FEB 19 CH.9 PE ASSESS MacBook Air D00 FI0 吕口 F3 F9 esc F5 F7 F2 ロ口 X
Suppose a 250. mL flask is filled with 0.80 mol of O2 and 0.30 mol of SO3. This reaction becomes possible: 2SO2(g) + O2(g) ~ 2SO3(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 r to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity.
The following reactions start at equilibrium.A stress is added and the position of equilibrium shifts. After the indicated stress is added which of the following reactions will proceed towards products?The added stress is the part listed inside the braces {} NH3(g) + HCl(g) NH4Cl(s) {and the volume is doubled} CO2(g) + H2(g) H2O (g) + CO (g) {and volume is reduced} Cl(s) + 2H2(g) CH4 {and a catalyst is added} N2(g) + 3H2(g) 2NH3(g) {and the volume is reduced}
Suppose that the equilibrium constant for the chemical reaction has an equilibrium constant of 2.3 x 107. What is the equilibrium constant for the reverse reaction?
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
Write the pressure equilibrium constant expression for this reaction. 2 H,(g)+O,(9)→2H,0(1)
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