Suppose a 250. mL flask is filled with 2.0 mol of NO,, 1.4 mol of CO and 0.40 mol of CO,, The following reaction becomes possible: NO,(g) + CO(g) NO(g) + CO,(s) The equilibrium constant K for this reaction is 0.676 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 1.64×10-3 moles of COCl2(g), 0.398 moles of CO, and 0.360 moles of Cl2 are at equilibrium in a 18.2 L container at 843 K, the value of the equilibrium constant, Kc, is .

Suppose a flask is filled with of and of . The following reaction becomes possible: The equilibrium constant for this reaction is at the temperature of the flask. Calculate the equilibrium molarity of . 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 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)

Suppose a 500. ml. flask is filled with 0.60 mol of Br₂, 0.70 mol of BrOCI and 0.20 mol of BrCl. The following reaction becomes possible: Br₂(g) +OCI, (8) BrOCI(g) + BrCI(g) The equilibrium constant K for this reaction is 7.17 at the temperature of the flask Calculate the equilibrium molarity of OCI, Round your answer to two decimal places. M

O KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 380.: NO,(8) + CO(3) = NO(g) + CO,(3) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.4 mol of NO, and 1.4 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little No, and CO. O There will be very little NO and CO,. O 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 = ] NO(9)+CO,(9) NO,(9)+CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] %3D 3 NO,(9)+3CO(g) 3 NO(g)+3CO,(9) 1L Explanation Check III

Suppose a 250. mL flask is filled with 0.20 mol of N, and 0.10 mol of NO. The following reaction becomes possible: N,(2) +O,(g) – -2NO(g) The equilibrium constant K for this reaction is 9.83 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places.

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II

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 ?

At a certain temperature, 0.88 mol N, and 2.654 mol H, are placed in a container. N2 (g) + 3H, (g) = 2NH; (g) At equilibrium, there is 0.82 mol NH, present. Determine the number of moles of N, and H, that are present when the reaction is at equilibrium. moles of N, at equilibrium: mol moles of H, at equilibrium: mol | privacy policy terms of use | help about us careers contact us O Ei A Gateway