This relationship between temperature and pressure is observed for any sample of gas confined to a constant volume. I find that temperature and pressure are linearly related. If the temperature on the kelvin scale increases by a certain factor, the gas pressure increases by the same factor. On the can is the warning “Store only at temperatures below 120 °F (48.8 °C). Do not incinerate.” The can contains an amount of isobutane gas at a constant volume, so if the temperature increased by heating, the pressure will increase proportionately. High temperature could lead to high pressure, causing the can to burst. Just like, The gas in the can is initially at 24°C, and the can has a volume of 350 mL. If we fill a balloon with air and seal it, If we put the balloon in a refrigerator, the gas inside gets cold and the balloon shrinks. If we make the balloon very cold, it will shrink a great deal, and it expands again when it warms up. Temperature is sometimes measured with a gas thermometer by observing the change in the volume of the gas as the temperature changes at constant pressure. A volume change caused by a temperature change at constant pressure means we should use Charles’s law. Decreasing the volume of a contained gas will increase its pressure, and increasing its volume will decrease its pressure. In fact, if the volume increases by a certain factor, the pressure decreases by the same factor, and vice versa. The earth’s atmosphere exerts a pressure, as does any other gas. Although we do not normally notice atmospheric pressure, we are sensitive to pressure change, for example, when your ears “pop” during take off and landing while flying, or when you dive underwater. Although the force of each collision is very small, any surface of appreciable area experiences a large number of collisions in a short time, which can result in a high pressure. In fact, normal air pressure is strong enough to crush a metal container when not balanced by equal pressure from inside the container. Atmospheric pressure is caused by the weight of the column of air molecules in the atmosphere above an object, such as the tanker car. At sea level, this pressure is roughly the same as that exerted by a full-grown African elephant standing on a doormat, or a typical bowling ball resting on your thumbnail. These may seem like huge amounts, and they are, but life on earth has evolved under such atmospheric pressure. If you actually perch a bowling ball on your thumbnail, the pressure experienced is twice the usual pressure, and the feeling is unpleasant.
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