Question

1. mark observes that magnesium reacts vigorously with hydrochloric acid, producing bubbles of hydrogen gas almost immediately. however, when he puts a piece of copper in hydrochloric acid, no reaction occurs.
2. for a chemistry demonstration, mr. lee drops a whole potato into hydrogen peroxide and observes that it reacts slowly, producing only a few bubbles. then he cuts the potato into small pieces and adds them to a fresh solution of hydrogen peroxide. this time, the reaction is much faster, producing bubbles rapidly.

part ii.

1. what are the two key requirements of collision theory for a successful reaction to occur?
2. give a real - life application of controlling the rates of reaction.

Explanation:

1. According to collision theory, for a successful reaction to occur, reactant particles must collide with sufficient energy (activation energy) and with the correct orientation.
2. One real - life application of controlling the rates of reaction is in the food preservation industry. Refrigeration slows down the chemical reactions (such as spoilage reactions) by reducing the kinetic energy of the molecules involved in the reactions. Another example is the use of catalysts in car engines (catalytic converters) to speed up the conversion of harmful pollutants (like carbon monoxide, unburnt hydrocarbons) into less harmful substances (carbon dioxide, water vapor) by providing an alternative reaction pathway with lower activation energy.

Answer:

1. Reactant particles must collide with sufficient energy (activation energy) and correct orientation.
2. Refrigeration for food preservation (slows down spoilage reactions) and catalytic converters in cars (speed up pollutant conversion reactions).