Using boyle's law and your understanding of what is happening at the particle level, explain why the pressure increases in aclosed water bottle as you squeeze it?

On particle level, temperature is a measure of the kinetic energy of the particles. By increasing the temperature, the particles hit the "walls" of the marshmallow with greater force, forcing...

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...

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...

Given this proportionality, $V_1/T_1=V_2/T_2$, where $T$ is in units of $"degrees Kelvin"$, and solve for $V_2$. $"Degrees Kelvin "=" Degrees Centigrade + "273.15*K$

Under conditions of low temperature, gases, all real gases, condense to give liquids. Under conditions of high pressure, the same condition obtains. Under moderate pressures and moderate to high temperatures,...

Clearly, if we pump in air into the football, the given assumption is invalid. For a full bladder (or whatever they fill footballs with these days), with a given quantity...

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....

According to the : $PV//T=PV//T$ This is just the general formula, and is derived from it. Boyle's Law says that temperature is constant. So, we can remove temperature from the...

This is a statement of Hess's Law using heats of formation. Here's a standard Hess's Law problem Calculate $ΔH^° "(reaction)"$ for the combustion of ammonia: NH₃(g) + ⁷/₄O₂(g) → NO₂(g)...