Law Theory Of Boyles's Law

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Theory:
Boyle’s Law states that when temperature (T) is kept constant, pressure (P) and volume (V) have an inversely proportional relationship. Boyle’s constant (B) can be expressed by V=B/Pwhere volume is (in this lab) cm^3 and pressure is in atm.

Charles’ Law states that when pressure is held constant, temperature and volume are directly proportional. Charles’ constant (C ) can be expressed by V=CTwhere volume is in cm^3 and temperature is in Kelvin.

Gay-Lussac’s Law states that when volume is held constant, temperature and pressure are directly proportional. Gay-Lussac’s constant (G) can be defined as P=GTwhere pressure is in atm and temperature is in Kelvin.

All three laws play a role in the ideal gas law, PV= nRT where P stands for pressure [atm], V is volume [L], n is the number of moles [mol], R is the gas constant [0.08206 atm*L/mol*K], and T is
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This makes volume the dependent variable and temperature the independent variable. The system volume was set by placing the piston about halfway through the cylinder to allow room for it to move up and down with the resulting volume change. The temperature was varied from a near-boiling temperature to a near-freezing temperature. The canister was placed into the water of the varied temperatures to change the temperature for the system. Each temperature changed the volume of the system as seen by the movement of the piston. The change in height was recorded and then that was used to calculate the new volume of the system. Following Charles’ Law, the volume increased as the temperature increased. This is shown in figure 2, the graph of volume vs temperature. To compare the experimental values to Charles’ Law, Charles’ constant was found using V = CT. The original volume of the system and room temperature were plugged in to find C, then various temperatures to find predicted

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