Homework Answers
a) false ( concentration of reactants may or may not be equal, but the concentration of reactants and products remain constant at equilibrium).
b) true
C) false
d) true.
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2. Label each of the following statement as True or False: Under chemical equilibrium, the concentration of the rea...
Laboratory 11, Equilibrium Control of a Reaction Name Chemical Equilibrlum: equilibrium is when the rates of...
Laboratory 11, Equilibrium Control of a Reaction Name Chemical Equilibrlum: equilibrium is when the rates of the forward and reverse reactions are equal. Therefore, the concentration of all reactants and products remain constant. This is not to say that the reaction has ceased. It is a dynamic situation at chemical equilibrium with the rate of disappearance of reactants the same as the rate of appearance of reactants through the reverse reaction (the same for the rate of disappearance and appearance...
Which of the following is a true statement about chemical equilibria in general? equilibrium [products] = [reactants].
Which of the following is a true statement about chemical equilibria in general? A. At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants]. B. Equilibrium is the result of the cessation of all chemical change. C. There is only one set of equilibrium concentrations that equals the Kc value. D. At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction. E. At...
Which of the following is true about the following chemical reaction at equilibrium? PICK ALL THAT...
Which of the following is true about the following chemical reaction at equilibrium? PICK ALL THAT APPLY. C6H12O6 + 6O2 6CO2 + 6H2O + Energy A. The concentration of H2O equals the concentration of O2. B. The rate of the forward reaction, reactants to products, equals the rate of the reverse reaction, products to reactants. C. The C-C bonds hold more energy in C6H12O6 than the C-O bonds in CO2. Hint: think teter-toter. D. The concentration of O2 is changing...
Which of the following is a true statement about chemical equilibria in general A
Which of the following is a true statement about chemical equilibria in general A.there is only one set of equilibrium concentrations that equal teh Kc value B.eqauilibrium is the result of cessation of all chemical change C.at equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction D.at equilibrium the total concentration of products equals the total concentration of reactants. that is [products]=[reactants] I am going with C. as correct can you confirm please...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward reaction stops only the reverse reaction stops both the forward and reverse reactions stop the rate constants for the forward and reverse reactions are equal the rates of the forward and reverse reactions are equal 2. A chemical equilibrium may be established by starting a reaction with reactants only. d. any quantities of reactants and products. products only. e. all the above equal quantities...
Which of the following statements are true in this equilibrium state? A. The concentrations of reactants...
Which of the following statements are true in this equilibrium state? A. The concentrations of reactants and prodcuts are still changing with time. B. The concentrations of reactants and products are equal. C. The rates of the forward and reverse reactions are equal. D. The rate of the reverse reaction is greater than that of the forward reaction. E. The rate of the forward reaction is greater than that of the reverse reaction.
Which of the following is true regarding the concentration of the reactants for a chemical reaction...
Which of the following is true regarding the concentration of the reactants for a chemical reaction that is at equilibrium. a. Concentration of the reactants will not change because the forward reaction has stopped b. Concentration of the reactants will not change because the intermediate is used up c. Concentration of the reactants will not change because the forward and reverse reacts rates are equal d. Concentration of the reactants will change because this is a dynamic process e. Concentration...
Learning Goal: Develop problem-solving skills wing chemical equilibria and oplying Le Chatter's principle Solving problems with...
Learning Goal: Develop problem-solving skills wing chemical equilibria and oplying Le Chatter's principle Solving problems with chemical equilibrium If you know the basic principles of chemical equilibrium, you can analyze and predict reversible reactions. To analyze any reversible reaction, follow these problem-solving steps: 1. Identify the reactants and products for the given chemical reaction. 2. Draw a diagram of the reaction to better understand what is happening 3. Identify how increasing or decreasing a product or reactant stresses the equilibrium...
QUESTION 1 12 pc The term chemical equilibrium # refers to a state of a reversiblo...
QUESTION 1 12 pc The term chemical equilibrium # refers to a state of a reversiblo • chemical reactions in which the rate # of the forward reaction is equal to the rate of the reverse reaction An equilibrium constant is a measure of the products • of a reaction Very high Kvalues mean that the concentration of products is high and for very, very high K-values it can be stated that a reaction is practically irreversible Very low K-values...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? (Hint: The equilibrium constant for the reaction is in the Background section.) Show your work 3. In the reaction below, NH3(g) + H2O(1) - NH; +H30+ the equilibrium constant is 10-34. Is this reaction likely to take place? Explain your answer. iron(III) and thiocyanate ions, the equilibrium expression...
Laboratory 11, Equilibrium Control of a Reaction Name Chemical Equilibrlum: equilibrium is when the rates of the forward and reverse reactions are equal. Therefore, the concentration of all reactants and products remain constant. This is not to say that the reaction has ceased. It is a dynamic situation at chemical equilibrium with the rate of disappearance of reactants the same as the rate of appearance of reactants through the reverse reaction (the same for the rate of disappearance and appearance...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward reaction stops only the reverse reaction stops both the forward and reverse reactions stop the rate constants for the forward and reverse reactions are equal the rates of the forward and reverse reactions are equal 2. A chemical equilibrium may be established by starting a reaction with reactants only. d. any quantities of reactants and products. products only. e. all the above equal quantities...
Learning Goal: Develop problem-solving skills wing chemical equilibria and oplying Le Chatter's principle Solving problems with chemical equilibrium If you know the basic principles of chemical equilibrium, you can analyze and predict reversible reactions. To analyze any reversible reaction, follow these problem-solving steps: 1. Identify the reactants and products for the given chemical reaction. 2. Draw a diagram of the reaction to better understand what is happening 3. Identify how increasing or decreasing a product or reactant stresses the equilibrium...
QUESTION 1 12 pc The term chemical equilibrium # refers to a state of a reversiblo • chemical reactions in which the rate # of the forward reaction is equal to the rate of the reverse reaction An equilibrium constant is a measure of the products • of a reaction Very high Kvalues mean that the concentration of products is high and for very, very high K-values it can be stated that a reaction is practically irreversible Very low K-values...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? (Hint: The equilibrium constant for the reaction is in the Background section.) Show your work 3. In the reaction below, NH3(g) + H2O(1) - NH; +H30+ the equilibrium constant is 10-34. Is this reaction likely to take place? Explain your answer. iron(III) and thiocyanate ions, the equilibrium expression...
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