1) When a mixture of potassium chlorate and an appropriate catalyst is heated in an open test tube, potassium chloride and oxygen gas are produced. This reaction is not reversible, because
a. the system reaches equilibrium
b. the reaction does not go to completion
c. the system is closed
d. the oxygen escapes
2) What happens to a reaction at equilibrium when a product concentration is decreased?
a. the reaction makes more products
b. the reaction makes more reactants
c. the reaction is unchanged
d. it is impossible to tell
Did you do the experiment with KClO3.What happened to the oxygen?
Le Chatelier's Principle, stated a little differently than the esoteric manner in which it is portrayed in texts, is this:
When a system in equilibrium is subjected to a stress,the reaction will try to undo what we've done to it. So if the PRODUCT is decreased, the reaction will try to ....
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1) b. the reaction does not go to completion
When a reaction goes to completion, it means that all of the reactants are converted into products. However, in this reaction, the reaction does not go to completion as there will always be some unreacted potassium chlorate left. This is because the reaction is not reversible, meaning the products cannot convert back into the reactants. So, even after heating, there will be some potassium chlorate remaining.
2) a. the reaction makes more products
According to Le Chatelier's principle, when a change is applied to a system at equilibrium, the system will respond by shifting in a direction that minimizes the effect of the change. In this case, when the concentration of a product is decreased, the system will respond by producing more products to counteract this decrease. This occurs in order to restore the equilibrium and maintain the balance between the reactants and products.
1) The correct answer is (d) the oxygen escapes. This reaction is not reversible because the oxygen gas produced during the reaction escapes from the open test tube. In a reversible reaction, the products can react to form the original reactants, but in this case, once the oxygen gas escapes, it cannot be converted back into the original reactants.
To arrive at this answer, we need to understand the concept of reversible and irreversible reactions. Reversible reactions can occur in both forward and backward directions, while irreversible reactions only proceed in one direction. In this case, the production of potassium chloride and oxygen gas from potassium chlorate is a one-way process because the oxygen gas escapes from the system.
2) When a reaction is at equilibrium and a product concentration is decreased, the reaction will shift in the direction that produces more of the product. Therefore, the correct answer is (a) the reaction makes more products.
To understand this, we can refer to Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change, it tries to counteract the change and shift the equilibrium position to reestablish equilibrium. In this case, by decreasing the concentration of a product, the system is disturbed, and to counteract this change, the reaction will shift in the direction that produces more of the product to restore equilibrium.