Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible:Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g)The equilibrium constant K for this reaction is 1.98 at the temperature of the flask.Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

Answered: Image /qna-images/answer/a5cabd65-3b29-4017-8136-dcce4214424d.jpg

Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) BrOCI(g) + BrC1 (g) 1 The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) BrOCI(g) + BrC1 (g) 1 The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

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...

See similar textbooks

Similar questions

At a certain temperature, the equilibrium constant K for the following reaction is 6.09 × 10 °: N,(3) + O,(g) =2 NO(g) Use this information to complete the following table. Suppose a 28. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N2 and O2. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2 NO(g) N3(9)+O2(9) 1L What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2N2(9)+20,(9) 4 NO(g)
Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?
Suppose a 500. mL flask is filled with 0.10 mol of Br₂, 0.70 mol of OC12 and 0.40 mol of BrOC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) ⇒ BrOC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 7.81 at the temperature of the flask. Calculate the equilibrium molarity of BrOC1. Round your answer to two decimal places. M X S
At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.
Suppose a 500. mL flask is filled with 1.8 mol of Cl,, 1.6 mol of CHCI, and 1.7 mol of HCl. The following reaction becomes possible: Cl,(g) +CHCI, (g) HCl(g)+CCl,(g) The equilibrium constant K for this reaction is 0.642 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places.
At a certain temperature, the equilibrium constant K for the following reaction is 0.0017: CO(g)+ H₂O(g) CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 27. L reaction vessel is filled with 1.5 mol of CO and 1.5 mol of H₂0. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. CO,(9)+H,(9) CO(g)+H,O(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 CO(g) + 2H₂O(g) 2 CO₂(g)+2H₂(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
Suppose a 500. mL flask is filled with 0.20 mol of Br,, 1.6 mol of OCl, and 1.9 mol of BrOCl. The following reaction becomes possible: 2' Br, (g) +OCl, (g)- BROCI(g)+BrC1(g) The equilibrium constantK for this reaction is 5.57 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. O M
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 ?
Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible: NO,(9) + CO(2) = No(g) + CO,(g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0.37 M ?
When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)
At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)
Help with the following question Please round the answer to 2 decimal places