As the temperature increases, the average kinetic energy of molecules increases. What would be the effect of an increase of temperature on pressure, provided the volume is constant? A.Increases B.Decreases C.Remains the same D.Becomes half
Hint: We are going to apply Gay Lussac’s law to explain the statement in the question, as Gay Lussac’s law shows the direct relationship between the pressure and the temperature of a fixed amount of gas at constant volume.
Complete step by step answer: Gay Lussac's law states that at constant volume, the pressure of a fixed amount of a gas is directly proportional to the temperature. Therefore, \[P \propto T\]………..at constant volume Thus, pressure increases if the temperature is increased at a constant volume. To elaborate more on this topic, we will see a real-life example. In hot summer days, we sometimes get the news of bursting of the inflated tires of vehicles. The bursting of tires explains to you about the Gay-Lussac's law. The inflated tires are under high pressure. When the temperature of the air rises, the pressure of the gas in the tubes increases. After an unbearable point, the tires ruptures or explodes. So, in this example, the volume of the gas or air in the tire tube remains constant. But with increasing atmospheric temperature, the pressure of the air also increases that ultimately results in the bursting of the tyre. Hence, the correct option is option A.
Note: We know that, as the particles are moving, they have kinetic energy. The faster they move, the more kinetic energy they will have. When a matter is hot, the particles will move faster and when it cools, the particles move more slowly.