# Question #8dc62

##### 1 Answer

#### Answer

#### Answer:

#### Explanation

#### Explanation:

Well, I can set things up for you to calculate the mass... but weight is in newtons,

**Normal Temperature and Pressure**, NTP, is apparently

The "mass" version of the **ideal gas law** can be derived.

#PV = nRT#

#n = (PV)/(RT)#

To get the units from

#nM -= m = (PVM)/(RT)#

In this case, we have:

#P# , pressure, in#"atm"# , of the ideal gas within the container.#V# , volume, in#"L"# , of the ideal gas.#M# , molar mass, in#"g/mol"# , of the ideal gas.#R = "0.082057 L"cdot"atm/mol"cdot"K"# , the universal gas constant.#T# , temperature, in#"K"# , within the container filled with ideal gas.

In case you couldn't tell, we're assuming ideal gases... So, the mass is:

#color(red)(m) = (cancel"1 atm" cdot 22.4 cancel"L" cdot M" g/"cancel"mol")/(0.082057 cancel"L"cdotcancel"atm""/"cancel"mol"cdotcancel"K" cdot (20 + 273.15 cancel"K"))#

#= color(red)(???)#

**Now, it's up to you to decide what the molar mass is.**

What is the molar mass of "nitrogen"? Is it

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