For the reaction choose the TRUE statement. 2 C2H6 (g) +7 O2 (g) = 4 CO2 (g) + 6 H₂O (g) Changing pressure will have no effect on the equilibrium. Increasing pressure will shift the equilibrium toward the reactants. Decreasing pressure will shift the equilibrium toward the reactants. Increasing pressure will shift equilibrium toward the products.

For the reaction choose the TRUE statement. 2 C2H6 (g) +7 O2 (g) = 4 CO2 (g) + 6 H₂O (g) Changing pressure will have no effect on the equilibrium. Increasing pressure will shift the equilibrium toward the reactants. Decreasing pressure will shift the equilibrium toward the reactants. Increasing pressure will shift equilibrium toward the products.

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 8QRT

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Similar questions

. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
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