As with many early scientific discoveries, the gas law referred to as was derived independently by many scientists, but Boyle received the credit for this law probably because he was the first to officially publish it in 1662.
Boyle's Law is an inverse relationship between pressure and volume. The kinetic theory of matter is fundamental to Boyle s Law. As the volume decreases the molecules collide more frequently...
It says that $Pprop1/V$...and thus it has NO FORMAL application to hot air ballooning...because pressure is formally constant. (Of course, as the balloon ascends, the atmospheric pressure DOES decrease...but to...
A basketball is held at a certain volume and pressure (constant temperature). When it hits the ground, the volume decreases and the pressure increases...and the increasing pressure springs the ball...
Well the original equation is PV = nRT From there, we can make several derivations If any part is constant, we can just isolate it and equal all of these...
states that the volume occupied by a gas and the pressure the gas exerts are inversely proportional: $P prop 1/V$ or $V prop 1/P$ Under constant temperature (and quantity...
According to , $color(red)(v prop1/p" "$when $" "color(green)(T" & "n$ constant. According to Charle's Law, $color(red)(v prop T" "$when $" "color(green)(p" "&" "n$ constant....
In volume and pressure vary inversely, whereas in , volume and pressure vary directly. Consider an example, if the pressure in Boyle's law is doubled from 1.0 atmospheres to 2.0...
tells us that for an ideal gas, at a constant temperature, volume is proportional to pressure. So doubling the volume, halves the pressure, providing temperature is kept the same....
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