17. When is a system at equilibrium said to be dynamic? * O just prior to equilibrium being established O at the start of the process when only reactants are present in the container when the system is changing at the molecular level with no change at the macroscopic level when the system is changing at the macroscopic level with no change at the molecular level O when the system reaches constant pressure

17. When is a system at equilibrium said to be dynamic? * O just prior to equilibrium being established O at the start of the process when only reactants are present in the container when the system is changing at the molecular level with no change at the macroscopic level when the system is changing at the macroscopic level with no change at the molecular level O when the system reaches constant pressure

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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Chapter 1 question 6: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 50.0L tank with 4.6 mol of ammonia gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.2 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.
In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the reactants is increased.
i See Periodic Table See Hin Increasing the concentration of a reactant shifts the position of chemical equilibrium towards formation of more products. What effect does adding a reactant have on the rates of the forward and reverse reactions? Choose one: O There is no effect on the forward and reverse reactions. For an equilibrium reaction, the forward and reverse rates are always equal. O Both the forward and reverse reactions speed up by the same amount. O The forward reaction speeds up immediately. As more product is made, the reverse reaction starts to speed up as the forward reaction starts to slow down until they are equal. O The forward reaction slows down initially. As the reaction proceeds, the reverse reaction slows down to meet the new forward reaction. O The forward reaction speeds up. Eventually, production of the product speeds up the reverse reaction rate to match the new forward rate. O It is impossible to say without more specific information.
In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the products is decreased.
When a reaction's reaction quotient is smaller than its equilibrium constant, what does this indicate about the reaction's equilibrium? The reaction must proceed in the reverse direction to return to equilibrium. The reaction is at equilibrium and will not change. O The reaction must proceed in the forward direction to return to equilibrium. O Nothing. There is no relationship between the reaction quotient and equilibrium constant.
4. Name two ways in which a system at equilibrium can be disturbed.
Two gaseous molecules react and produce two other gases molecules in an equilibrium reaction. What happens when the pressure is decreased? A it shifts to the right B more products form C It shifts to the left D Nothing happens
A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O
For the reaction at equilibrium: 2 H2O (g) +2 Cl2 (g) + energy 4 HCI (g) + O2(g), If a catalyst is added to the reaction mixture. The equilibrium will shift to the left. The equilibrium will shift to the right. The position of the equilibrium will not change.