Please help me Question: 1 When organic compounds containing sulfur are burned,

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Question: 1 When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2 formed can be determined by the reaction with hydrogen peroxide: H2O2(aq) + SO2(g) arrow H2SO4(aq) The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.479 g sample of coal is burned and the SO2 is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000 M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.

Explanation / Answer

Mole of NaOH used = 0.1000 x 28.44 x 10-3 moles = 2.844 x 10-3 moles

1 mole H2SO4 reacts with 2 moles of NaOH

So, 2.844 x 10-3 mole of NaOH reacts with (0.5 x 2.844 x 10-3 = ) 1.422 x 10-3 mole H2SO4

So, 1.422 x 10-3 mole of SO2 was produced from coal.

or, 64.066 x 1.422 x 10-3 = 4.55 x 10-2 g sulphur was present in 1.479 g of coal

Hence, Mass percentage of sulphur = (4.55 x 10-2 / 1.479 ) x 100 = 3.08 %

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