How do I find the mass of potassium in a $50.0 \cdot g$ $50.0*g$ mass of potassium sulfate?

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Answer 1 · 2015-09-07T15:51:16

Divide the mass by the molar mass.

Molecular mass $K_{2} {SO}_{4} = {174.26 g\cdotmol}^{- 1}$ $"K"_2"SO"_4 = "174.26 g·mol"^-1$ .

You can find this by adding the atomic masses of all the atoms that make up the molecule -- you can find these in the periodic table.

You have $50.0 g$ $"50.0 g"$ .

Divide the second value by the first.

$(50.0 color(red)(cancel(color(black)("g"))))/(174.26 color(red)(cancel(color(black)("g")))"·mol"^-1)= "0.287 mol"$ of $"K"_2"SO"_4$

Now remember to multiply this answer by $2$ , because there are two $"K"$ -atoms per molecule, so the final answer is $0.574mol$ of $"K"$

How do I find the mass of potassium in a 50.0*g50.0⋅g50.0*g mass of potassium sulfate?