Gay+Lussac+Kosky

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Gay-Lussac's Law
 * Gay-Lussac's law:** The pressure of a fixed mass of gas at a constant volume varies directly with the Kelvin temperature.So as the temperature increses, so does the pressure.

The energy and frequency of collisions depend on the average kenetic energy of the molecules. For every kelvin of temperature change, the pressure increases by 1/273 of the pressure at 0 degrees c.

P=kT or P/T=k (The value of T is the temperature in kelvins, and k is a constant that depends on the quantity of gas and the volume. For a given mass of gas at constant volume, the ratio P/T is the same for any set of pressure-temperature values.)

P1/T1=P2/T2 (P1 and T1 represent initial conditions. P2 and T2 represent a different set of conditions. When Values are known for three of the four quantities, the fourth value can be calculated for a system at constant volume.)

So, a sample problem would look like this.

You have a container with a pressure of 4atms and a temperature of 286 kelvins. What is the temperature of another container of the same volume with a pressure of 10 atms? Set it up like so: 1atm / 273 kelvins = 10 atms / ? (4atms/ 273 kelvins) / 10 atms= **2730 kelvins** In this figure we can see how not just temperature and pressure are related but also how that deals with volume