Pressure vs. Volume and Boyle’s Law
Pre-Lab Questions
According to our modern understanding of the gas laws, there are four measurable properties (variables) of a gas. These variables are P (pressure), V (volume), T (temperature), and n (number of moles). In Boyle’s experiment, which two variables were held constant?
Both the temperature (T) and the number of moles of gas (n) were held constant in Boyle’s experiment.
Fill in the blanks to summarize the relationship among the gas properties in Boyle’s experiment: For a fixed _________ of gas at constant ________, the ________ of a gas increases as the __________ of its container decreases.
For a fixed number of moles (n) of gas at constant temperature, the pressure of a gas increases as the volume of its container decreases.
Pressure is defined in physics as force divided by area (P = force/area). According to the kinetic-molecular theory, …show more content…
For a fixed number of moles (n) of gas at constant temperature, the pressure of a gas increases as the volume of its container decreases.
Pressure is defined in physics as force divided by area (P = force/area). According to the kinetic-molecular theory, the particles in a gas are constantly moving and colliding with the walls of their container. The pressure of the gas is related to the total force exerted by the individual collisions. Use the kinetic theory to explain the results of Boyle’s experiment.
In Boyle’s experiment, the pressure of air increased when it was compressed into a container that had a smaller volume. According to the kinetic theory, trapping gas particles in a smaller volume increases the number of collisions. Overall, due to this increase in collisions, the total force of the collisions with the container walls will
Pre-Lab Questions
According to our modern understanding of the gas laws, there are four measurable properties (variables) of a gas. These variables are P (pressure), V (volume), T (temperature), and n (number of moles). In Boyle’s experiment, which two variables were held constant?
Both the temperature (T) and the number of moles of gas (n) were held constant in Boyle’s experiment.
Fill in the blanks to summarize the relationship among the gas properties in Boyle’s experiment: For a fixed _________ of gas at constant ________, the ________ of a gas increases as the __________ of its container decreases.
For a fixed number of moles (n) of gas at constant temperature, the pressure of a gas increases as the volume of its container decreases.
Pressure is defined in physics as force divided by area (P = force/area). According to the kinetic-molecular theory, …show more content…
For a fixed number of moles (n) of gas at constant temperature, the pressure of a gas increases as the volume of its container decreases.
Pressure is defined in physics as force divided by area (P = force/area). According to the kinetic-molecular theory, the particles in a gas are constantly moving and colliding with the walls of their container. The pressure of the gas is related to the total force exerted by the individual collisions. Use the kinetic theory to explain the results of Boyle’s experiment.
In Boyle’s experiment, the pressure of air increased when it was compressed into a container that had a smaller volume. According to the kinetic theory, trapping gas particles in a smaller volume increases the number of collisions. Overall, due to this increase in collisions, the total force of the collisions with the container walls will