At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) ⟷⟷ (CH3)2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?   Group of answer choices the forward reaction will proceed in order to reestablish equilibrium. no change occurs. the equilibrium constant will increase. the reverse reaction will proceed in order to reestablish equilibrium.

Initial (M) Change (M) Equilibrium (M) -0.00875 0.0209 Consider the reaction of SO2 and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO2(g) + O₂(g) = 2 SO3(g) NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂2 at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 0.00875 re or pull up for additional resources 2.00 1 2SO2(g) 0.0216 2.00 0.0432 0.0148 + 0.0296 2 0.0041 O₂(g) 0.0175 0.0129 11 -0.0175 0.0061 2SO3(g) RESET 0.0350 0.0257

(Incorrect) 2 H₂S(g) + 2 H₂(g) + S₂(g) Kc = 9.3x 10-8 at 400°C 3.5 moles of H₂S are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of H₂ at equilibrium. 3.1 x 10-3 M (Your answer) 4.8 × 10-3 M 2.7 x 10-8 M 3.2 × 10-4 M 6.3 × 10-3 M (Correct answer)

1) Fill in the blanks below with appropriate reaction conditions or reaction products. H2, Pd HBr HBr ,hv OH OH

Consider this reaction at equilibrium. B(g) +2C(aq) 2D(g) The rates of the forward and reverse reactions are equal at equilibrium. There are 4 processes listed below that are applied individually to put a stress on the equilibrium. For each process, determine how that stress affects the rates of the forward and reverse reactions. Then drag the purple number that identifies the process to the gray arrow that will have the faster rate after that stress is applied There can be more than 1 number in each gray box. 1 Some B is added 3 Some D is added 2 Some C is removed 4 The volume of the gases is reduced. B(g) + 2C(aq) 2D(g)

Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. 2 H₂S(g) + SO₂(g) 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - x +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050- x 0.025 -3x 3 3 S(s) +3.x 0.050 - 2x -X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + x

On the basis of Kc for the following reaction, would you expect nearly complete reaction at equilibrium? 2H2(g) + O2(g) ↔ 2H2O(g);     Kc = 3x1081   Question 5 options:   Yes   No

When a product is added as a stressor on equilibrium, there is a(n): Group of answer choices increase in the forward reaction rate decrease in the forward reaction rate increase in the reverse reaction rate decrease in the reverse reaction rate

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CHEMWORK For the following endothermic reaction system at equilibrium: 2SO3(g) 2 2SO2(g) + O2(g) Choose the changes that will shift the equilibrium position to the right. (Select all that apply.) Decrease temperature Increase temperature Decrease volume Remove SO3(g) O Add SO2(g) Add a catalyst Add Ne(g)