# Can I use Boyle's law for a situation where the mass of the particles is held constant within a closed container and no chemical change occurs to these particles?

##### 1 Answer

Yes, the point is that the quantity of gas is fixed. Since you can convert between mass and

The ideal gas law has three common formulations:

#PV = nRT#

#PVM_m = mRT#

#PM_m = DRT#

where:

#P# is pressure in, say,#"atm"# or#"bar"# .#V# is volume in#"L"# .#n# is the#"mol"# s of gas.#M_m# is the molar mass of the gas in#"g/mol"# .#D# is the density in#"g/L"# .#m# is the mass in#"g"# .#R# is the universal gas constant. If it is units of#"L"cdot"atm/mol"cdot"K"# , then pressure is in#"atm"# . If it is in units of#"L"cdot"bar/mol"cdot"K"# , then pressure is in units of#"bar"# . And so on.#T# is the temperature in#"K"# .

You can interconvert between these.

#M_m * PV = M_m * nRT#

#=> color(blue)(PVM_m = mRT)#

#PVM_m * 1/V = m/VRT#

#=> color(blue)(PM_m = DRT)#

And furthermore, Boyle's law derives from the ideal gas law, so when the ideal gas law can use masses or

#P_1V_1 = nRT#

#P_2V_2 = nRT#

#=> color(blue)(P_1V_1 = P_2V_2)# ,

Boyle's Law