Which of the following statements concerning the reaction quotient Q and the equilibrium constant K is...
Which of the following statements concerning the reaction quotient Q and the equilibrium constant K is false?
As the temperature increases, the value of K always increases. Q must be equal to K at equilibrium.
By comparing the value of Q with K one can predict the direction of change for a system not initially in equilibrium.
The concentrations of pure solids and pure liquids are omitted from the expression for Q, because they do not change during the course of a chemical reaction.
The larger the value of K, the farther the forward reaction proceeds toward completion.
Homework Answers
The false statement is :
As temperature increases the rate constant k must always increase. This is not necessarily true because in order for this to remain true, the activation energy of reaction must be constant. Certain biological reaction have varying activation energy with temperature and beyond a certain temperature, the k value begins to decrease.
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Which of the following statements concerning the reaction
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