Consider the following equilibrium system: 2CrO4 2-(aq)+2H+(aq) 12 Cr2O72 (aq)+H2O(1) Write the equation for the equilibrium constant (K) of the reaction. The equilibrium constant (K) of the reaction above is K = 2.5 x 10-3, with initial concentrations as follows: [H+] = 1.0 x 10-2 M, [CrO4 2-] = 4.0 M, and [Cr2 072] = 1.0 x 10-4 M. If the concentration of the reactant H+was increased from1.0 x 10-2 M to 2.5 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift by comparing the value of Q to K. Q K, reaction will shift left Q=K, reaction is at equilibrium Q K, reaction will shift right
Consider the following equilibrium system: 2CrO4 2-(aq)+2H+(aq) 12 Cr2O72 (aq)+H2O(1) Write the equation for the equilibrium constant (K) of the reaction. The equilibrium constant (K) of the reaction above is K = 2.5 x 10-3, with initial concentrations as follows: [H+] = 1.0 x 10-2 M, [CrO4 2-] = 4.0 M, and [Cr2 072] = 1.0 x 10-4 M. If the concentration of the reactant H+was increased from1.0 x 10-2 M to 2.5 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift by comparing the value of Q to K. Q K, reaction will shift left Q=K, reaction is at equilibrium Q K, reaction will shift right
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 61QRT
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![Consider the following equilibrium system:
2CrO4 2-(aq)+2H+(aq) 12 Cr2O72 (aq)+H2O(1)
Write the equation for the equilibrium constant (K) of the reaction. The equilibrium
constant (K) of the reaction above is K = 2.5 x 10-3, with initial concentrations
as follows: [H+] = 1.0 x 10-2 M, [CrO4 2-] = 4.0 M, and [Cr2
072] = 1.0 x 10-4 M. If the concentration of the reactant H+was
increased from1.0 x 10-2 M to 2.5 M, calculate the reaction quotient (Q) and
determine which way the equilibrium position would shift by comparing the value of
Q to K.
Q<K, reaction will shift right
Q> K, reaction will shift left
Q=K, reaction is at equilibrium
Q<K, reaction will shift left
Q> K, reaction will shift right](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2a948ce4-bfec-4c4b-a693-d4721e6497c9%2F240a4cab-ad50-47fa-9ffb-5e85e0748129%2Fp57jfeq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following equilibrium system:
2CrO4 2-(aq)+2H+(aq) 12 Cr2O72 (aq)+H2O(1)
Write the equation for the equilibrium constant (K) of the reaction. The equilibrium
constant (K) of the reaction above is K = 2.5 x 10-3, with initial concentrations
as follows: [H+] = 1.0 x 10-2 M, [CrO4 2-] = 4.0 M, and [Cr2
072] = 1.0 x 10-4 M. If the concentration of the reactant H+was
increased from1.0 x 10-2 M to 2.5 M, calculate the reaction quotient (Q) and
determine which way the equilibrium position would shift by comparing the value of
Q to K.
Q<K, reaction will shift right
Q> K, reaction will shift left
Q=K, reaction is at equilibrium
Q<K, reaction will shift left
Q> K, reaction will shift right
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