The ideal gas law is a fundamental equation in thermodynamics which describes the relationship between the pressure (P), volume (V), temperature (T), and number of moles (n) of a gas. It is represented by the equation PV = nRT, where R is the universal gas constant.
To find pressure using the ideal gas law, you would rearrange the equation to solve for P. This would give you the formula P = nRT/V. Simply plug in the values for n, R, T, and V to calculate the pressure.
Absolute pressure is the total pressure exerted by a gas, including atmospheric pressure. It is measured relative to a perfect vacuum. Gauge pressure, on the other hand, is measured relative to atmospheric pressure and does not take into account atmospheric pressure.
According to the ideal gas law, as temperature increases, so does the pressure of a gas. This is because as temperature increases, the average kinetic energy of gas molecules also increases, causing them to collide with the container walls more frequently and with greater force, resulting in a higher pressure.
The SI unit for pressure is the Pascal (Pa). However, gas pressure is often measured in other units such as atmospheres (atm), millimeters of mercury (mmHg), or pounds per square inch (psi). These units can be converted to each other using conversion factors.