Boyle’s Law
Q1: What is Boyle’s Law?
Answer:
An Irish scientist of the 17th century, Robert Boyle, established Boyle’s Law, which affirms that, under constant temperature and amount of gas, the pressure and volume of a gas exhibit an inverse relationship to each other.
Q2: What is the formula for Boyle’s Law?
Answer:
The formula for Boyle’s Law is
P1V1 = P2V2
where
P1 is the initial pressure
V1 is the initial volume
P2 is the final pressure
V2 is the final volume
Q3: What is the significance of Boyle’s Law?
Answer:
Boyle’s Law has great significance as it explains the behavior of gases and serves as a fundamental principle for the study of thermodynamics. Additionally, it has numerous practical applications, including the design of engines and the compression of gases.
Q4: How is Boyle’s Law used in everyday life?
Answer:
The applications of Boyle’s Law is very evident in our everyday life, ranging from the inflation of balloons, working of the bicycle pump, and the functioning of scuba diving regulators all works on the principal of Boyle’s Law.
Furthermore, it finds extensive use in the compression of gases for various industrial and medical purposes.
Q5: How does temperature affect Boyle’s Law?
Answer:
An alteration in temperature affects Boyle’s Law due to the rise in the kinetic energy of gas particles leading to an increase in pressure. However, the validity of Boyle’s Law remains unaffected as long as the temperature is constant.
Q6: How does the amount of gas affects Boyle’s Law?
Answer:
Boyle’s Law is independent of the quantity of gas and holds true regardless of the amount of gas present, provided the temperature and volume remain constant.
Boyle’s Law
The English chemist Robert Boyle (1627–1691), widely regarded as one of the pioneers of the modern experimental science of chemistry, is commonly credited with this development. He found that increasing the pressure of a sample of contained gas by two times while holding its temperature constant reduced the gas volume by half. According to Boyle’s law, a gas’s volume changes inversely with pressure when the temperature is held constant. This is an illustration of an inverted relationship. The second variable drops when one variable rises in value.