Which of the following is the only way to change the equilibriumconstant?O change the volume of a solution with aqueous speciesO add a reactantO change the volume of a container with gaseous speciesO remove a reactantO change the temperatureO add a productO remove a product

Equilibrium constant (K) :- The ratio of product of equilibrium concentration of Products to…

Which of the following is the only way to change the equilibrium constant? change the volume of a solution with aqueous species add a reactant O change the volume of a container with gaseous species remove a reactant O change the temperature O add a product remove a product

Which of the following is the only way to change the equilibrium constant? change the volume of a solution with aqueous species add a reactant O change the volume of a container with gaseous species remove a reactant O change the temperature O add a product remove a product

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Select 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.
Decide 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.
QUESTION 4 Adding a catalyst to an equilibrium system will: produce more products at equilibrium. produce more reactants at equilibrium. not change the amount of reactants or products at equilibrium.
Which best shows that equilibrium has been reached? Question 4 options: The number of reactants is greater than the number of products The number of products is greater than the number of reactants The number of products is equal to the number of reactants The number of products varies little None of the above
Which of the following statements is FALSE: Group of answer choices The value of the equilibrium constant depends on the temperature Pure solids are not included in the equilibrium constant expression. At equilibrium, the reaction has stopped At equilibrium, the concentrations of all species are constant At equilibrium, the forward and reverse reactions are happening at the same rate
adding some CO(g) increasing the volume of the container removing some H₂O(g) Shifts in the direction of the products Shifts in the direction of the reactants chill the reaction removing H₂(g) as it forms Equilibrium does not change
If an equilibrium system has a high value (>1) for K, what does this indicate? How will the concentration of reactants compare to the concentration of products? [P] [R]
A Moving to another question will save this response. estion 3 For the following equilibrium reaction, hich cause and effect are correctly matched CO(g) + 2H2(g) CH 30H(g) heat add COshift left O remove H5, shift left O remove heat, no change O remove CH3OH, shift left O add heat, shift right