How do you calculate the ideal gas law constant?

How do you calculate the ideal gas law constant?

You do an experiment in which you measure the values of P,V,n, and T, and then you insert these values into the Ideal Gas Law.

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯∣∣aaPV=nRTaa∣∣−−−−−−−−−−−−−−−

You do an experiment in which you measure the values of %P, V, n%, and %T%, and then you insert these values into the Ideal Gas Law.

Explanation:

The Ideal Gas Law is%color(blue)(bar(ul(|color(white)(a/a)PV=nRTcolor(white)(a/a)|))) %where %R% is the Universal Gas Constant.We can rearrange this to get%R = (PV)/(nT)%The units of %R% depend on the units you use for %P% and %V%.For example, repeated experiments show that at standard temperature and pressure (STP) — 273.15 K and 1 bar — 1 mol of gas occupies 22.711 L.You can use this information to evaluate %R%.%R = (PV)/(nT) = (1 bar ×22.711 L)/(1 mol × 273.15 K) = 0.083 14 bar·L·K^-1mol^-1%If the pressure is measured in kilopascals (1 bar = 100 kPa), you calculate%R = (PV)/(nT) = (100 kPa × 22.711 L)/(1 mol × 273.15 K) = 8.314 kPa·L·K^-1mol^-1%If you use strictly SI units, then pressure is measured in pascals and volume is measured in cubic metres.%R = (PV)/(nT) = (100 × 10^3 color(white)(l)Pa × 22.711 × 10^-3 color(white)(l)m^3)/(1 mol × 273.15 K) = 8.314 Pa·m^3K^-1mol^-1%Always use the value of %R% that corresponds to the units that you are using for %P% and %V%.