Use Le Chatelier's Principle, Q, and K

Testing

For the following electrochemical half-reaction, the volume of the system is tripled. Towards which direction will the reaction proceed?

The hypothetical reaction is allowed to reach equilibrium in a sealed container. Suddenly, heat is added and the volume changes from  to due to an outside force. In which direction will the equilibrium shift?

When the following reaction occurs in a sealed flask, the surface underneath the flask heats up. Which direction will the equilibrium shift if the temperature is increased? 

The following reaction is run with and without a platinum catalyst. In which reaction will the value of be greater?

In the following reaction, the partial pressures of hydrogen and oxygen at a certain time were measured to be and ,respectively. In which direction will the reaction proceed if for this reaction?

If all concentrations in the following reaction are found to be at equilibrium and the concentration of sodium hydroxide is increased by , which direction will the reaction proceed?

In a given reaction if , which side of the reaction will be favored?

The dissolution of table salt in water depends on temperature. At the salt will only slightly dissolve; whereas at , the salt will totally dissolve. What happens to the equilibrium when the temperature is increased from to ?

Consider the endothermic reaction below.

If we increase the temperature of the reaction, what will happen to the equilibrium?

If the temperature of a reversible exothermic reaction is increased, in which direction will the equilibrium shift?

The values of and for the reaction below are and , respectively. 

Consider the following conditions.

1. At , the concentrations of hydrogen acetate and sodium acetate are both while the pressure of carbon dioxide is . 

2. At , the concentrations of hydrogen acetate and sodium acetate are and , respectively, while the pressure of carbon dioxide is . 

Given the above conditions, at which condition is sodium bicarbonate at a higher concentration?

A sealed container with the following reaction is allowed to expand to double its initial volume. In which direction will the reaction proceed?

The following reaction takes place in a sealed container. If the pressure is decreased, what happens to the equilibrium?

For the following reaction, the conditions below are found to be true:

1. At equilibrium, .

2. At some other time, , and the concentration of oxygen gas is found to be . 

What is the concentration of hydrogen gas and in which direction will the reaction proceed? The reaction is as follows.