Chemistry: High School: 9th and 10th Grade Quiz - Reversible and Irreversible Reactions (Questions)

This Chemistry quiz is called 'Reversible and Irreversible Reactions' and it has been written by teachers to help you if you are studying the subject at high school. Playing educational quizzes is a user-friendly way to learn if you are in the 9th or 10th grade - aged 14 to 16.

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There are many types of different chemical reactions: neutralization, decomposition, combustion and oxidation are four of the common ones. This high school Chemistry quiz is all about reversible and irreversible chemical reactions. When a reaction is described as being reversible, it can go both forwards and backwards at the same time. These type of reactions occur when the products are able to react with each other or if the product is decomposed by the conditions used for the reaction. A good example is the decomposition of ammonium chloride. The products are ammonia and hydrogen chloride. Ammonia is a base, hydrogen chloride is an acid and they react together to form ammonium chloride.

NH₄Cl ⇌ NH₃ + HCl

When you see a reaction written down using a double arrow between the reactants and products, it means that it is reversible. A single arrow indicates an irreversible reaction.

When talking about reversible reactions, you will hear the phrase dynamic equilibrium used. This describes the situation in a closed system when the forward and reverse reactions are taking place at exactly the same rate - the concentration of products and reactants remain the same. In a closed system, no products or reactants can escape or be lost from the reaction vessel - it is fully sealed. At equilibrium, the reactions are both still happening but everything is balanced. This balance can be changed either by altering the conditions or by adding/removing a reactant or product.

In any reversible reaction it is the forward portion that we want, so we must change the conditions to be as favorable as possible. You studied this in detail when you were learning about the Haber process. If the forward reaction is exothermic for example, the reverse reaction will be endothermic by exactly the same amount. Increasing the temperature means that there is more heat available which helps the reverse reaction (remember that endothermic reactions absorb energy (usually heat) from the surroundings, so if there is more heat energy available it can be more readily absorbed). We say that the equilibrium shifts to the left. In other words, the backwards reaction is favored and less product is made. Cool down the system and the opposite will be true as it will be easier for the forward exothermic reaction to lose energy to the surroundings.

Try this quiz and see how well you understand reversible and irreversible chemical reactions.