QUESTION 2 Which of the following statements about a system at chemical equilibrium is true? O The forward and reverse reactions both stop. O The forward reaction has a faster rate than the reverse reaction. O The reverse reaction has a faster rate than the forward reaction. O The forward reaction rate is equal to the reverse reaction rate. O There are no more reactants left.

QUESTION 2 Which of the following statements about a system at chemical equilibrium is true? O The forward and reverse reactions both stop. O The forward reaction has a faster rate than the reverse reaction. O The reverse reaction has a faster rate than the forward reaction. O The forward reaction rate is equal to the reverse reaction rate. O There are no more reactants left.

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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"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
What happens to a system when products are added to a reaction vessel? O The amount of products increases. O The amount of reactants increases. O The amount of reactants decreases. O The system remains at equilibrium.
Question 43 The following reaction is a reversible reaction. Which of the following statements best describes what it means for this reaction to be reversible? HCOOH+H,O - HCOO + HẠO* O a. This reaction only occurs in the reverse direction as written above. O b. All of the reactant molecules react to make product and then all of the product molecules react to make reactants again. c. Forward and reverse reactions proceed at the same rate. O d. Forward and reverse reactions occur simultaneously. Oe. The rate of the reverse reaction is must faster than the rate of the forward reaction.
Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the reactant concentrations drop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the product concentrations rise. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the forward rate constant drops.
MULTIPLE CHOICE Question 11 What does Le Châtelier's principle state? A Equilibrium cannot be re-established once it is disturbed. B A system at equilibrium will remain at equilibrium forever. A system will react to re-establish equilibrium if it is disturbed. A reaction will proceed to completion if equilibrium is disturbed.
Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.
According to Le Châtelier's principle, how will an increase in concentration of a reactant affect the equilibrium system? Shift it toward the products Shift it toward the reactants Shift it toward the side with higher total mole concentration or Shift it toward the side with lower total mole concentration
23. What happens when a chemical reaction reaches equilibrium? The amounts of reactants and products remain constant because the reaction stops. The reaction stops because the concentration of reactants is too low to sustain it. The reaction reverses so some of the products are converted back into reactants. The rate of the forward reaction is the same as the rate of the reverse reaction. PREVIOUS 23 of 25 NEXT REVIEW
Question 20 Which statement best describes general equilibrium? Equilibrium is reached when the reaction stops. There is only one set of equilibrium concentrations that equals the Kc value. At equilibrium, the rate of the forward reaction is the same as the rate of the reverse reaction. At equilibrium, the total concentration of products equals the total concentration of reactants.
4. What does a bi-directional arrow tell you about a chemical reaction? The reaction happens only once The reaction happens more than once The reaction is able to reverse O The reaction is at equilibrium
For questions 19-25. Consider the following exothermic reaction at equilibrium: N2(g) - 3H2(g) = 2NH3(g). Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablish. What will happen to N2? 24. Decrease the volume (constant T) * increase decrease no reaction
Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g) heat + 4NO(g) + 6H2O(g) b) heat + 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g)