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$\overline{)\mathbf{mass}\mathbf{}\mathbf{percent}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{element}}{\mathbf{total}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{compound}}\mathbf{\times}\mathbf{100}}$

For the percent by mass C, we’re going to rewrite the equation as:

$\overline{)\mathbf{mass}\mathbf{}\mathbf{percent}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{C}}{\mathbf{mass}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}\mathbf{SO}}\mathbf{\times}\mathbf{100}}$

Mass of C:

2 x 12.01 g/mol = 24.02 g/mol

Molar mass of C_{2}H_{6}SO:

C: 2 x 12.01 g/mol = 24.02 g/mol

H: 6 x 1 .01 g/mol = 6.06 g/mol

S: 1 x 32.07 g/mol = 32.06 g/mol

O: 1 x 16.00 g/mol = 16.00 g/mol

What is the mass % of carbon in dimethylsulfoxide, C_{2}H_{6}SO?

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Based on our data, we think this problem is relevant for Professor Barclay's class at LONESTAR.