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The gas argon is a noble gas that is chemically inert. It has the lowest boiling point of any gas, at -185 degrees Celsius. The density of argon varies with temperature and pressure, but in general it can be calculated as follows: Argon Gas Density = (2 * T/P) * Rho_T + Rho_P where, assuming ideal behavior: T = temperature in Kelvin P = pressure in Pascal’s (Pa) Rho_t and Rho_p are the gas constants for argon at T and P respectively. The relationship between these two is given by: Rho_t*(273+T/293)=0.001196367RHOP + 0.00279480366RHOHO – 354 RHOLN where RHOLN=24325.*ln((273+298)/323), so that if you know one of the other variables, you can calculate it as follows: RHOP=(-354)*RHOHLN/(RT)+360; or alternatively use this calculator which also allows the input of a RHOHLN value. This equation is valid for any three-dimensional pressure and temperature, but because argon has such low molecular mass it only becomes significant at high pressures where its density can be significantly greater than that predicted by ideal gas behavior. For example: At atmosphere (101325 Pa) and T=0 degrees Celsius, Argon Gas Density = .0087 g/l or 0.0870 ozm^-nbsp;per cubic foot which differs from experimentally measured values of about .0014g/l due to the non-ideal nature of this noble gas’s behaviour under these conditions; while at 100 atmospheres and higher, Argon Gas Density will usually exceed


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