Behavior of Gases
Student: Mary Chrisin L. ObreroDate: October 7, 2014
Section: 116
Behavior of Gases and Determination of Absolute Zero
Experiments 4&5
Introduction: First of all, the Boyle’s law (pressure-volume law) indicates that the volume of a certain amount of gas given held at a constant temperature differentiates inversely with the applied pressure when there are constant temperature and mass. Equations: PV=C. When pressure goes up, volume goes down (derived from the equation above): P1V1 = P2V2 = P3V3. Furthermore, this particular equation dictates that the product of the initial volume and pressure is equal to the product of the volume and pressure after a change under constant temperature. On the other hand, Charles’ law states that the volume of a given amount of gas held at a constant pressure is considered directly proportional to the Kelvin temperature. Equations: V T or V / T = C. Therefore, as the volume rises, the temperature goes up, as well, and vice versa. Same as the Boyle’s law, initial and final volumes, and temperatures under constant pressure can be calculated also. V1 / T1 = V2 / T2 = V3 / T3. Last but not least, the Gay-Lussac’s law emphasizes that the pressure of a given amount of gas held at a constant volume is said to be directly proportional to the Kelvin temperature. Equations: P T. As the pressure rises, the temperature also rises, vice versa. Like the other gas laws mentioned above, this law’s initial, final volumes, and temperatures under constant pressure can also be calculated. Meanwhile, temperature is the measurement of the kinetic energy of particles inside of a certain object. Thus, the object will increase in temperature if particles have a high amount of kinetic energy. Meanwhile, the object will decrease in temperature if the particles have less kinetic energy. Nonetheless, an object with the lowest temperature tends to have particles that are not moving at all. Last but not least, this particular temperature depicts
Section: 116
Behavior of Gases and Determination of Absolute Zero
Experiments 4&5
Introduction: First of all, the Boyle’s law (pressure-volume law) indicates that the volume of a certain amount of gas given held at a constant temperature differentiates inversely with the applied pressure when there are constant temperature and mass. Equations: PV=C. When pressure goes up, volume goes down (derived from the equation above): P1V1 = P2V2 = P3V3. Furthermore, this particular equation dictates that the product of the initial volume and pressure is equal to the product of the volume and pressure after a change under constant temperature. On the other hand, Charles’ law states that the volume of a given amount of gas held at a constant pressure is considered directly proportional to the Kelvin temperature. Equations: V T or V / T = C. Therefore, as the volume rises, the temperature goes up, as well, and vice versa. Same as the Boyle’s law, initial and final volumes, and temperatures under constant pressure can be calculated also. V1 / T1 = V2 / T2 = V3 / T3. Last but not least, the Gay-Lussac’s law emphasizes that the pressure of a given amount of gas held at a constant volume is said to be directly proportional to the Kelvin temperature. Equations: P T. As the pressure rises, the temperature also rises, vice versa. Like the other gas laws mentioned above, this law’s initial, final volumes, and temperatures under constant pressure can also be calculated. Meanwhile, temperature is the measurement of the kinetic energy of particles inside of a certain object. Thus, the object will increase in temperature if particles have a high amount of kinetic energy. Meanwhile, the object will decrease in temperature if the particles have less kinetic energy. Nonetheless, an object with the lowest temperature tends to have particles that are not moving at all. Last but not least, this particular temperature depicts