CHEM 1&2 Lab Manual & worksheets pg 127

CHEM 1&2 Lab Manual & worksheets pg 127 -...

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Experiment 10: Gas Laws General Chemistry I and II Lab Manual Dakota State University Page 127 of 232 Boyle’s law relates gas volume to pressure. Boyle carefully measured how the volume of a gas changes as he varied the pressure on that gas. He discovered that for a system with a fixed amount of gas (n) and temperature (T), a plot of volume versus pressure gave a straight line with a negative slope. A more common way to state this would be to say that as pressure increases, volume decreases. We say that for constant n and T, volume is inversely proportional to pressure; The vertical line above with the subscript “n,T” is a mathematical symbolism used to remind us that this is true only if the number of moles of the gas n and the temperature T remain constant. A proportionality can be converted into an equation with the introduction of some constant, in our case k, even if we do not know the value of this constant.
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Unformatted text preview: Thus, or, since k must be constant, 2 2 1 1 P V P V = for any two states 1 and 2 (that is, for any initial state 1 to any final state 2 where we vary either pressure or volume. Charles decided that he was rather more interested in the relationship between the volume of a gas and the temperature of the gas at constant number of moles n and pressure p. Holding the pressure constant on the cylinder (as simple as not adding any weight to the cylinder, making its pressure equal to atmospheric pressure), he measured the volume of a gas as he heated and cooled the cylinder. Charles discovered on plotting volume and temperature that there was a direct proportionality, that is, as temperature increased, so increased volume. He wrote the corresponding proportionality as The next step, as with Boyle, is to remove the proportionality by adding a constant; | 1/P V T n, a | k = VP T n, | k/P = V T n, | T V P n, a...
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