Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G

Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G

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 0.30 mol of Br,, 1.5 mol of OCl, and 1.0 mol of BrOCl. The following reaction becomes possible: Br, (g) +OCl, (g) – BROC1(g) +BrC1(g) The equilibrium constant K for this reaction is 0.214 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. do Ar OM ?
Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible: NO2(g)+CO(g) NO(g)+CO2(g) The equilibrium constant K for this reaction is 9.16 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. please check your work. most people get this wrong!
Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.
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Suppose a 500.mL flask is filled with 1.5mol of CO, 1.1mol of H2O and 1.6mol of H2. The following reaction becomes possible: CO(g)+H2O(g)+CO2(g)+H2(g) The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 924.: CO(g) + H₂O(g) → CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 17. L reaction vessel is filled with 0.75 mol of CO₂ and 0.75 mol of H₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. CO₂(g) + H₂(9) CO(g)+H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 CO(g) + 3H₂O(g) P 3 CO₂(g) + 3H₂(9) There will be very little CO and H₂O. There will be very little CO2 and H₂. Neither of the above is true. K = 0 K = 0 ■ x10 X ? 00. Ar 8.
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At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?
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