A plot of pressure vs temperature for low density gases is as follows: When extrapolated the lines will meet the temperature axis at

Question

A plot of pressure vs temperature for low density gases is as follows: When extrapolated the lines will meet the temperature axis at (A) -100° C (B) -173° C (C) -273.15° C (D) will meet at different points

Tardigrade Admin · Accepted Answer

From the ideal gas equation, P V=n R T. Holding the volume of a gas constant, given ρ propto T . The absolute minimum temperature for an ideal gas, inferred by extrapolating the straight line to the axis is found to be -273.15° C and is designated as absolute zero.

Q. A plot of pressure vs temperature for low density gases is as follows: When extrapolated the lines will meet the temperature axis at

$- 10 0^{\circ} C$

$- 17 3^{\circ} C$

$- 273.1 5^{\circ} C$

will meet at different points

From the ideal gas equation, $P V = n RT$ . Holding the volume of a gas constant, given $ρ \propto T .$ The absolute minimum temperature for an ideal gas, inferred by extrapolating the straight line to the axis is found to be $- 273.1 5^{\circ} C$ and is designated as absolute zero.

Q. A plot of pressure vs temperature for low density gases is as follows: When extrapolated the lines will meet the temperature axis at

−100∘C

−173∘C

−273.15∘C

will meet at different points

From the ideal gas equation, PV=nRT. Holding the volume of a gas constant, given ρ∝T. The absolute minimum temperature for an ideal gas, inferred by extrapolating the straight line to the axis is found to be −273.15∘C and is designated as absolute zero.

$- 10 0^{\circ} C$

$- 17 3^{\circ} C$

$- 273.1 5^{\circ} C$

From the ideal gas equation, $P V = n RT$ . Holding the volume of a gas constant, given $ρ \propto T .$ The absolute minimum temperature for an ideal gas, inferred by extrapolating the straight line to the axis is found to be $- 273.1 5^{\circ} C$ and is designated as absolute zero.