Equilibrium and Le Chateliers Principle Q

Complete the two acid dissociation reactions for the ethylenediammonium ion and select the correct symbol for the equilibrium constant for each reaction. Step 1: NHẸCH,CH,NH(aq) — What is the symbol for the equilibrium contant for step 1? O Kb2 O Ka2 Ο Και Kbl Step 2: NH₂CH₂CH₂NH3(aq) = What is the symbol for the equilibrium constant for step 2?

Le Chatelier's Principles Complete the following chart by writing left, right or none for equilibrium shift, and decreases, increases or remains the same for the concentrations of reactants and products, and for the K value. N2(g) + 3H2(g) ↔2NH3(g) + 22.0 kcal Stress Equilibrium Shift [N2]  [H2]  [NH3]  K Add N2           Add H2           Add NH3           Remove N2           Remove H2           Remove NH3           Increase Temperature            Decrease Temperature            Increase Pressure            Decrease Pressure

According to Le Chatelier's Principle, a reaction at equilibrium will attempt to stay at equilibrium, even if stresses are applied. Which of the following is NOT a stress that chemical reactions respond to?        A decrease in the concentration of an aqueous or gaseous reactant.       A change in temperature.       An increase in the concentration of an aqueous or gaseous product.       A change in pressure when gaseous reagents are nonexistent.       A change in pressure when gases are present in differing mole amounts on each side of the equation.

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Which statement about chemical equilibrium is not true? Chemical equilibrium can only be attained by starting with reagents from the reactant side of the equation. At equilibrium, the reactant and product concentrations are constant. The same equilibrium state can be attained starting either from the reactant or product side of the equation. At equilibrium, the reactant and the product concentrations show no further change with time. At equilibrium, the forward reaction rate equals the reverse reaction rate.

Given the following equilibrium equation: CH4(g) + 2O2(g) CO2(g) + 2H₂O(g) + heat What would be the effect of Removing O₂ from the reaction mixture. No effect and CO₂ concentration goes down. Shifts to the left and CO2 concentration increases. Shifts to the right and H₂O concentration increase. Shifts to the left and CH4 concentration increases.

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

Chapter 1 question 7 There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. +CaC2s2H2Ol ⇌ +C2H2gCaOH2s K1 +6C2H2g+3CO2g4H2Ol ⇌ 5CH2CHCO2Hg K2 The net reaction is: +6CaC2s+16H2Ol3CO2g ⇌ +6CaOH2s5CH2CHCO2Hg K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2.

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LPG with bromine  Get one tube containing LPG and quickly add a few drops of bromine  Replace the cork immediately to prevent the escape of the gas  Shake the tube and observe for the appearance of a precipitate  Test for the presence of HBr with a blue litmus paper moistened with distilled water and held with tweezers. What are your observations? What is the appearance of the precipitate? Did the blue litmus paper changed in color?

18) In one of your experiments, you used a Grignard reaction to make a carboxylic acid. „Br 1) Mg 2) CO2 As part of this experiment, the following procedures were given: 1. When the Grignard reaction begins to slow down, place 10 g of crushed dry ice in a 150 mL beaker. Do not take time to weigh the dry ice. Use approximately the amount in the beaker indicated by your instructor. The CO2 is in large excess and will not affect your calculation of percent yield of benzoic acid product. Cover the beaker with a watch glass. 2. When most of the magnesium has reacted and the ether boiling subsides, quickly pour the contents of the tube into the beaker containing dry ice. 3. Add a few milliliters of ether to the test tube and swirl to rinse. Add the rinse liquid to the beaker. 4. Cover the beaker with the watch glass and allow it to stand until the next lab period. During the interim, the excess dry ice will have sublimed. 5. Hydrolyze the Grignard addition product by slowing adding 30 mL of…

1. For a solution equilibrium, if the concentration of a product is decreased, Kc will also decrease. Group of answer choices True False   2. Which of the following is the factor that causes a reversible chemical reaction to reach equilibrium? Group of answer choices Reaction stopped. The forward and reverse reaction rates become equal. the concentrations of the reactants and products have become equal. Reactants are used up.

Can you help me with number 3 part A, number 3 part B, number 3 part C, and number 3 part D?

Resarch project( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering add lots of pictures and details

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1. When adding a reagent as indicated for each equilibrium shown below, predict whether it will shift to the left, right, or unchanged. Equilibrium CaF2(s) Ca²+ + 2F CaF2(s) Ca²+ 2F- HCN H+ + CN HCN 3 H+ + CN HCN 3 H+ + CN Reagent Added CaCl₂ KF KCN HCI KC1 Shifting Direction 2. Predict the shifting direction of the equilibrium 2SO3(g) = 2SO₂(g) + O₂(g) under each of the following added condition changes, where the standard enthalpy change is AH = 197.78 kJ/mol. a. Increasing the temperature. b. Increasing the pressure. C. Adding O₂ when the reaction is at equilibrium. d. Removing O2 from the system at equilibrium.

Resarch project ( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering Ocean Acidification add lots of pictures and details

Classify the conditions given as indicating that a reaction is at equilibrium, is not at equilibrium, or that the conditions may occur in either state. At equilibrium Not at equilibrium May or may not be at equilibrium Answer Bank The products and reactants have equal concentrations. The concentration of products is greater than the concentration of reactants. The concentrations of products and reactants are constant. The forward reaction is occurring at a very slow rate. The concentration of reactants is slowly increasing. The forward and reverse reactions occur at equal rates.

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Write the basic equilibrium equation for C,H,NH, 3. O4- D2. O+ n2+ O3+ O4+ 1 2 3 4 7 8 1 3 4 5 O6 (s) (1) (g) (aq) + -> H C OH Reset • a H,O Delete 80 888 F3 F4 F5 F6 F7 FB 2# $ % & * 3 4 5 6 7 9 W E R Y U CO

Which one shows an exothermic reaction? Both are exothermic II Neither are exothermic I

According to Le Chatelier's Principle, a reaction at equilibrium will attempt to stay at equilibrium, even if stresses are applied. Which of the following is NOT a stress that chemical reactions respond to? A) A change in pressure when gaseous reagents are nonexistent.   B) A change in temperature.   C) An increase in the concentration of an aqueous or gaseous product.   D) A decrease in the concentration of an aqueous or gaseous reactant.   E) A change in pressure when gases are present in differing mole amounts on each side of the equation.

Classify each compound by reactivity. Acidic oxide Basic oxide Acid salt Salt Acid Base Answer Bank H3PO4 Bao Na20 CO2 N2O5 Ca(OH)2 K2HPO4 KI NazSO4

Would this equation shift left or right?

When you add HCl to a solution containing aqueous sodium acetylsalicylate (structure shown below), a precipitate formed. Which is the structure of this precipitate?

Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. Reactants are transformed into products even at equilibrium. At equilibrium the forward rate constant equals zero. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the product concentrations rise. As a reaction proceeds forward toward equilibrium the reverse rate rises.

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Can you help me with number 2? Can you explain it to me?

In this Chemical Reaction at equilibrium: N H 3 + H B r ⟺ N H 4 + + B r − If you upset the equilibrium by adding NH3, what will happen to the reaction equilibrium.

Ccan you help me every step by step? Can you help me with number 2 part A and number 2 part B?