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P V = n R T P = pressure in atm V = volume in liters n = moles R = proportionality constant = 0.08206 L atm / mol · K T = temperature in Kelvins. Ideal Gas Law. Holds closely at P < 1 atm. Ideal Gases.

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ideal gas law
PV=nRT

P= pressure in atm

V = volume in liters

n = moles

R = proportionality constant

= 0.08206 L atm/ mol·K

T = temperature in Kelvins

Ideal Gas Law

Holds closely at P < 1 atm

ideal gases
Ideal Gases

Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory.

  • Gases consist of tiny particles that are far apart
  • relative to their size.
  • Collisions between gas particles and between
  • particles and the walls of the container are
  • elastic collisions
  • No kinetic energy is lost in elastic
  • collisions
ideal gases continued
Ideal Gases (continued)
  • Gas particles are in constant, rapid motion. They
  • therefore possess kinetic energy, the energy of
  • motion
  • There are no forces of attraction between gas
  • particles
  • The average kinetic energy of gas particles
  • depends on temperature, not on the identity
  • of the particle.
real gases do not behave ideally
Real Gases Do Not Behave Ideally

Real gases DO experience inter-molecular attractions

Real gases DO have volume

Real gases DO NOT have elastic collisions