For the reaction: 2NOCl(g)  ⟷⟷   2NO(g) + Cl2(g) If the reaction were allowed to reach equilibrium and you were to remove some Cl2(g), what would happen? [Check all that are correct.] Group of answer choices - Equilibrium would shift to the right. - Equilibrium would shift to the left. - The amount of NOCl(g) would increase. - The amount of NO(g) would increase.

choose ONE of each of the red selections. for example you choose between endothermic or exothermic and fill out the other options to make the statement true

The equilibrium                         4 NH3(g) + 4 O2(g)  ⇆  2 N2O (g) + 6 H2O(l)           ΔHo = −142 kJ/mol Is established in a sealed container with a piston. Which of the following actions will increase the amount of the products present at equilibrium?             I    Increasing the volume of the container             II   Reducing the volume of the container             III  Removing some of the H2O(l) from the container             IV  Adding some NH3(g) to the container             V   Adding N2(g) to the container             VI  Raising the temperature             VII Lowering the temperature

For the reaction: 2H2(g) + CO(g)  ↔↔   CH3OH(g) If the reaction were allowed to reach equilibrium and you were to increase the pressure, what would happen? [Check all that are correct.] Group of answer choices - Equilibrium would shift to the right. - Equilibrium would shift to the left. - The amount of H2 would increase. - The amount of CO would increase. - The amount of CH3OH would increase.

. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2

The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Kc? Cl₂(g) + H₂O(g) = 2 HCl(g) + 1/2 O₂(g) K = 7.52 × 10-2 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) OK= 5.66 x 10-3 OK= 13.3 OK= 0.150 OK = 177 OK = 3.65 K = ?

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.

For the following reaction at equilibrium, which of the changes below would cause the equilibrium to shift to the right and form more products? 2 NOBR(g) + 2 NO(g) + Br2(g) A H°n = 30 kJ/mol Increase the temperature Increase the container volume Remove some NO Add some NOBr

The diagrams represent the equilibrium mixture for the reaction X, (g) + Y(g) = X(g) + XY(g) at 300 K and 500 K. The X atoms are represented using red spheres, and the Y atoms are represented using blue spheres. Is the reaction exothermic or endothermic? exothermic cannot determine from the diagrams 300 K endothermic 500 K