Boyle S Law Lab F13
Name: _____________________________________ Block: _________ Date: _______________
Lab #14: Boyle’s Law Objective: To determine the relationship between the pressure and volume of a gas at constant temperature.
Introduction:
The relationship of pressure to volume for a gas in a rigid container was first described in 1662 by the Irishborn scientist Sir Robert Boyle (16271691), and is known as Boyle's Law. As long as the temperature of the gas remains constant, the pressure of a gas has a predictable relationship with the volume of the gas.
The pressure of a gas is a measure of the force the gas exerts on the walls of its container. Recall that the particles (atoms or molecules) of the gas are in constant motion, colliding with each other and with the walls of their container. The net effect of these collisions is pressure. Even if a gas is not contained, the force of collisions results in pressure. For example, the air around us exerts a force on every object it touches, and we can measure this atmospheric pressure with a barometer.
In this activity, you will use a datalogger (called a SPARK) and a Pressure Sensor connected to a syringe full of air to investigate the relationship between the volume and pressure of a gas.
Procedure:
Part A. Measuring Air Pressure
Follow PART A of the SPARK directions in order to determine the pressure of air in the room in four different units (kilopascals, atmospheres, millimeters of Hg, and torr). Record your results in your lab notebook.
Part B. Boyle’s Law
Follow Part B of the SPARK directions in order to obtain the pressure as the volume of air is changed from
60 to 20 milliliters in 5 mL increments. Record your results.
Analysis:
1. Using your data, construct a neat line graph of pressure (y) vs. volume (x).
MPHS Chemistry
2. For each data point that you measured, find the product of
Lab #14: Boyle’s Law Objective: To determine the relationship between the pressure and volume of a gas at constant temperature.
Introduction:
The relationship of pressure to volume for a gas in a rigid container was first described in 1662 by the Irishborn scientist Sir Robert Boyle (16271691), and is known as Boyle's Law. As long as the temperature of the gas remains constant, the pressure of a gas has a predictable relationship with the volume of the gas.
The pressure of a gas is a measure of the force the gas exerts on the walls of its container. Recall that the particles (atoms or molecules) of the gas are in constant motion, colliding with each other and with the walls of their container. The net effect of these collisions is pressure. Even if a gas is not contained, the force of collisions results in pressure. For example, the air around us exerts a force on every object it touches, and we can measure this atmospheric pressure with a barometer.
In this activity, you will use a datalogger (called a SPARK) and a Pressure Sensor connected to a syringe full of air to investigate the relationship between the volume and pressure of a gas.
Procedure:
Part A. Measuring Air Pressure
Follow PART A of the SPARK directions in order to determine the pressure of air in the room in four different units (kilopascals, atmospheres, millimeters of Hg, and torr). Record your results in your lab notebook.
Part B. Boyle’s Law
Follow Part B of the SPARK directions in order to obtain the pressure as the volume of air is changed from
60 to 20 milliliters in 5 mL increments. Record your results.
Analysis:
1. Using your data, construct a neat line graph of pressure (y) vs. volume (x).
MPHS Chemistry
2. For each data point that you measured, find the product of