Applying Le Châtelier's Principle 12 of 22 <> N Review | Constants | Periodic Table Consider the following system at equilibrium: D(aq) + E(aq) 2F(aq) When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help Increase (D] If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the Decrease [F] Decrease (E) Decrease (D] Increase (F] stress. Triple (D] and reduce [E] to one third Triple both (E] and (F] Increase (E] Leftward shift Rightward shift No shift

Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: HF (aq)+H,O(1)→F (aq)+H;O (aq) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 1.12 g H,0 762. g F 0.380 g H,0* 0.393 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K - | Check Explanation 2021 McGraw-Hill Education. All Rights Reeserved 23

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What is the correct expression for the equilibrium constant K? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a с [B] [H₂O] [BH+][OH-] [B] [BH+][OH-] [BH+][OH- [B] [BH+][OH [B] [H₂O]

Use the given equilibrium constant to identify it's corresponding chemical equation assuming every reactant and product are in the gas phase.   Keq = ([NH3]4[O2]3)/([N2]2[H2O]6)

What is chemical equilibrium and what kind of reactions are in equilibrium (what is their equilibrium constant?) Write the equilibrium expression for the following reactions: • H2 + O2 ------ 2 H2O   CH4 + 2O2 ------ CO2 + 2 H2O   6 CO2 + 6H2O ------ C6H12O6 + 6O2

# 4, 5, and 6

Write the equilibrium expression for the following equilibrium: A+2B 3C+D

s) Consider the following reaction at equilibrium. State the effect that each of the following would have on equilibrium H₂CO(g) →H*(aq) + HCO₂ (aq) a) adding NaHCO₂ b) increasing T c) Adding NaOH AH<0

Can you help me every step by step with number 3 part A,  part B, part C, part D? Can you explain it to me?