+Imagine 212. mmol of HCH,CO, are removed from a flask containing a mixture of HCH,CO,, H,O, H,O' and CH,CO, at equilibrium, and then answer thefollowing questions.Zero.What is the rate of the forwardGreater than zero, but less than the rate of the reverse reaction.reaction before any HCH3CO2 hasbeen removed from the flask?Greater than zero, and equal to the rate of the reverse reaction.Greater than zero, and greater than the rate of the reverse reaction.Zero.What is the rate of the forwardGreater than zero, but less than the rate of the reverse reaction.reaction just after the HCH3CO2 hasbeen removed from the flask?Greater than zero, and equal to the rate of the reverse reaction.Greater than zero, and greater than the rate of the reverse reaction.Zero.What is the rate of the forwardGreater than zero, but less than the rate of the reverse reaction.reaction when the system has againreached equilibrium?Greater than zero, and equal to the rate of the reverse reaction.Greater than zero, and greater than the rate of the reverse reaction.None.How much less HCH3CO2 is in theflask when the system has againreached equilibrium?Some, but less than 212. mmol.212. mmol.More than 212. mmol.

Le Chatelier's Principle : If an equilibrium is subjected to stress, the equilibrium shifts in such…

Imagine 212. mmol of HCH,CO, are removed from a flask containing a mixture of HCH,CO,, H,O, H,0' and CH,CO, at equilibrium, and then answer the following questions. Zero. What is the rate of the forward reaction before any HCH3CO2 has been removed from the flask? Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward reaction just after the HCH3CO2 has Greater than zero, but less than the rate of the reverse reaction. been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward reaction when the system has again reached equilibrium? Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. None. How much less HCH3CO2 is in the flask when the system has again reached equilibrium? Some, but less than 212. mmol. 212. mmol. More than 212. mmol.

Imagine 212. mmol of HCH,CO, are removed from a flask containing a mixture of HCH,CO,, H,O, H,0' and CH,CO, at equilibrium, and then answer the following questions. Zero. What is the rate of the forward reaction before any HCH3CO2 has been removed from the flask? Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward reaction just after the HCH3CO2 has Greater than zero, but less than the rate of the reverse reaction. been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward reaction when the system has again reached equilibrium? Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. None. How much less HCH3CO2 is in the flask when the system has again reached equilibrium? Some, but less than 212. mmol. 212. mmol. More than 212. mmol.

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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part d and e
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1
Part A It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following: Determine the value of the equilibrium constant, Kpal, for the reaction • When a reaction is reversed, its K value is inverted; that is, Kreverse = 1/Kforward- • When the coefficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor. • When reactions are added, their K values are multiplied. CO2 (g) = C(s) + 02(g). Kgoal =? by making use of the following information: 1. 2CO2 (g) + 2H20(1) = CH3COOH(1) + 202(g). K1 = 5.40 x 10-16 2. 2H2(g) + O2(g) = 2H,O(1). K2 = 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g). K3 = 2.68 x 10 9 Express your answer numerically. • View Available Hint(s) V ΑΣφ Kgoal = Submit Part B Determine the equilibrium constant, Kroal, for the reaction 4PCI, (g) = P4(s) + 10Cl2 (g), Kgoal =? by making use of…
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