At a particular temperature, 8.0 moles of NO2 is placed into a 1.0-L containe and the NO2 dissociates by the reaction 2 NO2(g) → 2 NO(g) + O2(g) At equilibrium the concentration of NO(g) is 1.0 M. Calculate K for this reaction.

1. Given the equilibrium constant values N₂ (g) + ¹/2O₂(g) → N₂O (g) N₂O4 (g) → 2 NO₂ (g) ½ N₂(g) + O₂(g) → NO₂ (g) Kel=2.7 x 10-18 K₂=4.6 x 10-³ K3 = 4.1 x 10⁹ Determine the value of K. for the reaction below: 2 N₂O(g) + 30₂ (g) → 2 N₂O4 (g)

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H₂(g) + 1₂(g) 2 HI(g) Kc = 53.3 At this temperature, 0.300 mol H₂ and 0.300 mol I₂ were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium?

At a particular temperature, K = 1.00 x 10² for the reaction H₂(g) +1₂(g) → 2HI(g) In an experiment, 1.00 mol H₂, 1.00 mol 12, and 1.00 mol HI are introduced into a 1.00 L container. Calculate the equilibrium concentrations of all reactants and products.

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)

2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) The system initially contained 0.2500 M NO, 0.1300 M H2, and 0.2500 M H₂O. At equilibrium, the concentration of NO is 0.1296 M. What is the equilibrium concentration of H₂? [H₂] = [?] x 10¹ M K= [N₂] [H₂O]2 [NO]2[H₂]2 Coefficient (green) Exponent (yellow) Enter

The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5,   0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

A student ran the following reaction in the laboratory at 316 K:2CH2Cl2(g) CH4(g) + CCl4(g)When he introduced CH2Cl2(g) at a pressure of 0.487 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be 0.219 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. 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. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA