Suppose a 500. mL flask is filled with 1.8 mol of 12 and 1.5 mol of HI. The following reaction becomes possible:H2(g) +I2(g)2HI(g)The equilibrium constant K for this reaction is 0.782 at the temperature of the flask.Calculate the equilibrium molarity of HI. Round your answer to two decimal places.MG

[HI] = 1.56 MExplanation:The problem asks for the equilibrium concentration of HI for the…

Answered: Suppose a 500. mL flask is filled with…

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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At a certain temperature, 0.820 mol SO3 is placed in a 3.50 L container. 2 SO₂ (g) ⇒ 2 SO₂(g) + O₂(g) 3 At equilibrium, 0.170 mol O₂ is present. Calculate K. Kc =
Suppose a 250. mL flask is filled with 0.10 mol of N, and 1.8 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) == 2NO (g) The equilibrium constant K for this reaction is 0.422 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. IM ?
Suppose a 500. mL flask is filled with 1.5 mol of Cl2 and 0.60 mol of HCI. The following reaction becomes possible: H2(g)+ Cl2(g) 2HCl (g) The equilibrium constant K for this reaction is 3.73 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places. Ом
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Suppose a 250. mL flask is filled with 0.70 mol of H2 and 1.1 mol of 12. The following reaction becomes possible: H2(g) +I2(g) — 2HI(g) =0 The equilibrium constant K for this reaction is 8.37 at the temperature of the flask. Calculate the equilibrium molarity of 12. Round your answer to two decimal places. Ом
Suppose a 500. mL flask is filled with 0.30 mol of H, and 1.4 mol of HI. This reaction becomes possible: H,(2) +I,(g) = 2HI(s) 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 I,. You can leave out the M symbol for molarity. H, HI initial change equilibrium Continue Submi O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Priva
Suppose a 500. mL flask is filled with 0.20 mol of N2 and 1.6 mol of NO. The following reaction becomes possil N2(g) + O2(g) 2NO(g) The equilibrium constant K for this reaction is 0.205 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Шм ✗
Suppose a 500. mL flask is filled with 1.5 mol of H₂ and 1.2 mol of Cl₂. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 3.45 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M Ś
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