Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- when an equilibrium is disrupted (“stressed”) due to changes that a chemist imposes on the system, Le Chatelier’s Principle predicts that the equilibrium will shift in the direction that will undo as much of the change as possible. For instance, if a particular reactant compound is removed through some chemical means, then the equilibrium will shift to favor the reactants, so as to replace some of the lost compound. In this lab, you will observe the effects of stress on the tetrachlorocobaltate(II)/hexaquocobalt(II) equilibrium shown below: CoCl42-(solv) + 6 H2O(solv) Co(OH2)62+(solv) + 4 Cl-(solv) blue pink The (solv) means a solvated species. In this system, ethanol is the solvent. This means that water can not be excluded from the reaction quotient any longer, since it is now a solute in ethanol and therefore has a measurable concentration. The color of the solution provides a visual clue about the dominant cobalt species…arrow_forwardIf the equilibrium constant for an equilibrium system has decreased because of a "stress", how have the concentrations changed? O [reactants] and [products] decreases [reactants] decreases and [products] increases O [reactants] increases and [products] decreases [reactants] and [products] increasesarrow_forwardCan you show me how to answer this type of question I found on a online practice organic chemistry review.arrow_forward
- Explain Le Chatelier's principle as it relates to chemical equilibrium. Describe the types of stresses that cause chemical reactions and equilibrium to make more products. Use details to support your answerarrow_forwardSelect all the TRUE statements about chemical equilibrium. At equilibrium the rates of the forward and reverse reactions are equal. At equilibrium the concentrations of reactants and products remain constant. At equilibrium the reactants are still being converted to products (and vice versa). At equilibrium the concentrations of reactants and products are equal.arrow_forwardWhich is the appropriate description to show the effect of a catalyst on the reaction rate and equilibrium in a reversible reaction: Reactants › Products O• The rate of the forward reaction is increased. • The rate of the reverse reaction is decreased 0 •The equilibrium position is displaced to the right O • The rate of the forward reaction is increased. The rate of the reverse reaction is increased The equilibrium position is unchanged. • The rate of the forward reaction is increased. 0 •The rate of the reverse reaction is unchanged • The equilibrium position is displaced to the right • The rate of the forward reaction is unchanged. The rate of the reverse reaction is unchanged The equilibrium position is unchanged. Suppose that an exothermic reaction, Reactants < › Products, is at equilibrium. According to Le Chatelier's Principle, if the reaction temperature is increased, in which direction will the equilibrium be displaced? O The equilibrium will be displaced toward the…arrow_forward
- Increasing the concentration of the reactants will slow down the reaction. O true O falsearrow_forwardLabel the following statements as true or false.True False When Q < Kc, the reaction shifts to the left to reduce stress on the system. True False When a system is at equilibrium, the reactants and the products of the reaction will be equal in concentration. True False When a system is at equilibrium, the reaction rate of the forward reaction is less than to the reaction rate of the reverse reaction. True False When Q > Kc, the reaction shifts to the right to reduce stress on the system. True False For a reversible reaction, the ΔH of the forward reaction is equal in magnitude but opposite in sign to the ΔH of the reverse reaction. True False If Kc=5 for the reaction A + B <--> AB, then AB <--> A + B has a Kc=0.2arrow_forwardSolid carbon dioxide is also called dry ice. Dry ice is placed in a sealed container. Some CO2 sublimes and the following equilibrium is formed: CO2 (s) = CO2 (g) If the amount of solid CO2 (dry ice) in the container is doubled what would happen? (Hint: Write the equilibrium constant expression.) Solid carbon dioxide is also called dry ice. Dry ice is placed in a sealed container. Some CO2 sublimes and the following equilibrium is formed: CO2 (s) = CO2 (g) If the amount of solid CO2 (dry ice) in the container is doubled what would happen? (Hint: Write the equilibrium constant expression.) The amount of CO2 (g) would increase, but not double. The amount of CO2 (g) would double. The partial pressure of CO2 (g) would increase. The amount of CO2 (g) would not change.arrow_forward
- 1) When a system is at equilibrium: A) the reaction rate of the forward reaction is equal to the rate of the reverse B) the reaction rate of the reverse reaction is small compared to forward C) the reaction rate of the forward reaction is small compared to the reverse D) the amount of product and reactant is exactly equal 2) What will be the equilibrium expression for this reaction? (DO NOT INCLUDE SOLID PRODUCTS, THEIR CONCENTRATION IS ALWAYS EQUAL TO 1.) 4 CuO (s) + CH4 (g) = CO2 (g)+ 4 Cu (s) + 2 H2O (g) A) [CuO]/[Cu] B) [CuO]4/[Cu]4 C) [Cu]4/[CuO]4 D) [CO2][H20]2/[CH4] 3) Which K value below corresponds to the system with the highest proportion of reactants? А) К 3D25 B) K = 0.067 C) K = 1.5 x 10-3 D) K 3D 1.2 х 103arrow_forwardSelect 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 reverse rate equals zero.At equilibrium the speed of a reaction equals its rate constant.As a reaction proceeds forward toward equilibrium the reverse rate rises.At equilibrium the rate of change of product concentration is zero.arrow_forwardDecide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.arrow_forward
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