2.404 g of a compound were burned in oxygen and found to produce only 3.520 g CO₂(g),2.564 g SO₂(g)and 1.440 g H₂O(l).Determine the empirical formula of the compound.

Question

Quizplus · Accepted Answer

1) Calculate the moles of each product: - moles of CO₂(g) = 3.520 g / 60.07 g/mol = 0.0586 mol - moles of SO₂(g) = 2.564 g / 64.06 g/mol = 0.0400 mol - moles of H₂O(l) = 1.440 g / 98.08 g/mol = 0.0147 mol 2) Determine the lowest whole number ratio of moles by dividing all values by the smallest value: - 0.0147 mol / 0.0147 mol = 1 - 0.0400 mol / 0.0147 mol = 2.72 - 0.0586 mol /0.0147 mol = 3.99 3) Round the ratios to the nearest whole number: - 1:2:4 4) Write the empirical formula using the ratios as subscripts: - C₂SH₄

2404 G of a Compound Were Burned in Oxygen and Found