NEW
Font size
WorksheetsBoyle’s Law
Total questions: 15
Worksheet time: 15mins
What happens to air bubbles exhaled by a diver as they ascend?
They shrink in size
They expand as pressure decreases
They remain the same size
They increase in density
If a diver’s lungs contain 2L of air at the surface (1 atm), what will the volume be at a depth of 10 meters (2 atm)?
4 L
2 L
1 L
0.5 L
What is the key outcome of Boyle’s Law experiments?
Volume decreases as temperature increases
Volume remains constant at high pressure
Volume is inversely proportional to pressure
Volume is directly proportional to pressure
What happens to gas molecules in the lungs during ascent if air isn’t exhaled?
The molecules expand, leading to overinflation of the lungs
The molecules condense, reducing lung volume
The pressure inside the lungs decreases
The volume of the gas remains constant
Which mathematical expression represents Boyle’s Law?
P × V = k
P + V = k
P/V = k
P – V = k
A diver’s lung volume expands from 6L to 30L during ascent. What does this indicate about pressure at depth?
Pressure at depth is lower
Pressure at depth is higher
Pressure at depth equals surface pressure
Volume and pressure are unrelated
What happens to gas concentration as surrounding pressure increases?
It decreases
It increases
It remains constant
It fluctuates
Which factor is directly proportional to the volume of a gas in Boyle's Law?
Temperature
Pressure
Reciprocal of pressure
The number of gas molecules
Why is it dangerous to hold your breath during ascent after breathing compressed air?
The air will expand, causing lung overinflation
The air will shrink, reducing oxygen levels
The lungs will fill with water
The pressure will remain constant
What is the formula for Boyle's Law?
P1V1=P2V2
P1V1/P2V2
P1V2=P2V1
P1/V1=P2/V2
The relationship of which two variables are compared in Boyle's Law?
pressure & volume
volume & temperature
temperature & pressure
volume & moles (amount of gas)
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
12.9 L
0.72 L
7.2 L
3.44 L
A gas occupies 3 liters at a pressure of 2 atm. According to Boyle's Law, what will be the volume if the pressure is increased to 6 atm?
1 liter
2 liters
0.5 liters
6 liters
Which of the following real-world applications is an example of Boyle's Law?
A balloon expanding as it rises in the atmosphere
A car engine converting fuel into energy
Water boiling at a lower temperature at high altitudes
Ice melting into water
In an experiment demonstrating Boyle's Law, a gas is compressed from 8 liters to 4 liters. If the initial pressure was 1 atm, what is the final pressure?
0.5 atm
1 atm
2 atm
4 atm
