Calculate the pressure in millimeters of mercury exerted by 0.123 moles of an ideal gas that occupies a volume of 45.1 mL at 52.0 °C. What is the name of the gas law used in this calculation?
calculation?

GASES

Before working with gases some definitions are needed:

PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg

TEMPERATURE: Kelvin, K, which is o

C + 273

STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)

BOYLE'S LAW (temperature is constant): PV = constant

This is an inverse relationship: if one variable increases the other must

decrease.

CHARLES' LAW (pressure is constant): V = constant x T

This is a direct relationship: if one variable increases so does the other.

GAY-LUSSAC'S LAW (volume is constant): P = constant x T

This is a direct relationship: if one variable increases so does the other.

IDEAL GAS LAW: PV = nRT, where

P = pressure of the gas sample

V = volume of the gas sample

T = Kelvin temperature of the gas sample

n = moles of the gas sample

R = molar gas constant

AVOGADRO'S LAW: At the same temperature and pressure, equal volumes of all

gases have the same number of molecules. At STP one mole of any gas occupies a

volume of 22.4 L: this is the molar volume

Explanation:

is this helpful ? it just a example

the volume increases