Keq for the reaction 2 NO2 (g) N204 (g) is 4.73. If a container holds 2.10 M N2O4 and 0.0887 M NO2 and is allowed to come to equilibrium, which of the following would be the BEST set-up to solve for the concentration of NO2 at equilibrium? NO2 N204 I: 0.0887 2.10 C: +2X - 1X E: 0.0887 + 2X 2.10 - 1X NO2 N204 1: 0.0887 2.10 C: - 2X + 1X E: 0.0887 2X 2.10 +1X NO2 N204 I: 0.0887 C: - 2 X E: 0.0887- 2X 2.10 +1X NO2 N204 : 0.0887 2.10 C: +1X 1X E: 0.0887 + 1X 2.10 2X NO2 N204 I: 0.0887 2.10 C: + 1X 2X E: 0.0887 + 1X 2.10 - 1X

Consider the equilibrium reaction below: N₂(g) + O₂(g) 2 NO(g) Create an equilibrium constant, K, expression for the above reaction using the drag and drop tools: K= [N₂][0₂] [N₂]+[0₂] [NO]² [N]²[O]² [NO] 2[NO]

The following reaction has an equilibrium constant Ke = 1.5. A, + B, =2AB The following diagrams represent reaction mixtures where A is represented by red spheres and B is represented by blue spheres. For each diagram, determine if the reaction mixture is at equilibrium. If it is not at equilibrium, determine the direction in which the reaction will proceed to reach equilibrium.

The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(g)+ H2O(1)-2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 6.6 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 8.7 g H₂O 230.3 g HNO, 10.8 g NO 10.3 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 I Don't Know Submit 5 ? olo 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

You place 4.57 mol of dinitrogen trioxide, N2O3, into a flask, where it decomposes at 25.0°C and 1.00 atm. N2O3(g)  NO2(g) + NO(g) What is the composition of the reaction mixture at equilibrium if it contains 0.59 mol of nitrogen dioxide, NO2?N2O3(g)  molNO2(g)  molNO(g)  mol

Consider the following system at equilibrium where AH 2NOBr(g) 2NO(g) + Br₂ (9) O increases O decreases O remains the same The value of Qc O is greater than Ke is equal to Ke O is less than Ke If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke The reaction must O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. = The number of moles of Br₂ will O increase O decrease O remain the same 16.1 kJ, and K = 6.50 × 10-³, at 298 K: -3

Consider the following system at equilibrium: N₂(g) + 3H₂(g) = 2NH3(g); AH = 92.94 kJ Which of the following changes will shift the equilibrium to the right? Lincreasing the temperature II.decreasing the temperature III increasing the volume IV.decreasing the volume Vremoving some NH3 VLadding some NH3 VII removing some N₂ VIII. adding some N₂ O II, III, V, VIII O I, III, V, VII OI, VI, VIII OLIV, V, VIII O II, IV, V, VIII

If this reaction is taking place in a 1.0L container, and 1.5 mol of SO2 were added to the reaction, whatwill the new concentrations of all fours gases be when equilibrium is reestablished?