What mass of sulfur gas would be found in a 2.45 liter container at SATP?

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What mass of sulfur gas would be found in a 2.45 liter container at SATP?

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Answer 1 · 2017-06-29T01:53:52

$3.21$ $3.21$ $g S$ $"g S"$

Explanation:

We're asked to to find the mass of gaseous sulfur that occupies a volume of $2.45$ $2.45$ $L$ $"L"$ at standard ambient temperature and pressure.

I'll assume for these purposes that the sulfur is present as individual, gaseous atoms, rather than $S_{8}$ $"S"_8$ (which is reasonable considering $S_{8}$ $"S"_8$ is a solid at these conditions).

Standard ambient temperature and pressure (SATP) is defined as

$298.15$ $298.15$ $K$ $"K"$ (temperature; equal to ${25.0}^{o} C$ $25.0^"o""C"$ )
$1$ $1$ $atm$ $"atm"$ (pressure)

We can use the ideal-gas equation to solve for the number of moles of sulfur, $n$ $n$ , knowing that the gas constant, $R$ $R$ is equal to $0.082057 \frac{L ∙ atm}{mol ∙ K}$ $0.082057("L"•"atm")/("mol"•"K")$ :

$P V = n R T$ $PV = nRT$

$n = (PV)/(RT) = ((1cancel("atm"))(2.45cancel("L")))/((0.082057(cancel("L")•cancel("atm"))/("mol"•cancel("K")))(298.15cancel("K")))$

$= color(red)(0.100$ $color(red)("mol S"$

Now, let's use the molar mass of sulfur, $32.07$ $"g/mol"$ , to calculate the number of grams:

$0.100cancel("mol S")((32.07color(white)(l)"g S")/(1cancel("mol S"))) = color(blue)(3.21$ $color(blue)("g S"$

Thus, if a $2.45$ - $"L"$ tank is filled with pure gaseous sulfur at SATP, we can expect the sulfur sample to have a mass of $color(blue)(3.21$ $sfcolor(blue)("grams"$ .

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What mass of sulfur gas would be found in a 2.45 liter container at SATP?

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