# A sample of hydrogen gas occupies a volume of 33.4 L at STP. How many moles of hydrogen gas is this?

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Feb 9, 2018

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If we *ASSUME* (!!!!) that hydrogen gas is an ideal gas, then we *ASSUME* that the **ideal gas law** works:

#PV = nRT#

#P# is pressure in#"atm"# or#"bar"# ...#V# is volume in#"L"# .#R = "0.083145 L"cdot"bar/mol"cdot"K"# #=# #"0.082057 L"cdot"atm/mol"cdot"K"# is the universal gas constant.#T# is the temperature in#"K"# .#n# is obviously the mols of IDEAL gas.

And so,

#n = (PV)/(RT)#

STP is defined **since** 1982 as **before** 1982 as

**Before** 1982,

#n = ("1 atm"cdot"33.4 L")/("0.082057 L"cdot"atm/mol"cdot"K" cdot "273.15 K")#

#=# #"1.49 mols"#

But since we're not old-timers who are stuck in the past, we look at **AFTER** 1982 to obtain:

#n = ("1 bar" cdot "33.4 L")/("0.083145 L"cdot"bar/mol"cdot"K" cdot "273.15 K")#

#=# #ulcolor(blue)"1.47 mols"#

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Victoria E.
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Feb 9, 2018

At STP, all gases have a molar volume of 22.4 L/mol

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