Question

Quantitative analysis shows that a compound contains 32.38% sodium, 22.65% sulfur and 44.99% oxygen. Find the empirical and molecular formula given that the molar mass is 275.

Answer 1

Answer:n2so4

Explanation:the answer is in below slide pls check and write thank you

Answer 2

Answer:

To find the empirical formula, we need to convert the percentages of each element into grams and then into moles.

Assuming a 100-gram sample, we have 32.38 g of sodium, 22.65 g of sulfur, and 44.99 g of oxygen.

Converting these masses into moles using their respective atomic masses (22.99 g/mol for Na, 32.06 g/mol for S, and 16.00 g/mol for O), we get approximately 1.41 moles of Na, 0.71 moles of S, and 2.81 moles of O.

Explanation:

We need to divide each mole value by the smallest mole value to obtain the simplest whole-number ratio between them. In this case, the smallest mole value is 0.71 mol (corresponding to S), so dividing all mole values by this number gives us approximately 2 moles of Na, 1 mole of S, and 4 moles of O.

• The empirical formula is Na2SO4 (two sodium atoms, one sulfur atom, and four oxygen atoms).

• To find the molecular formula from the empirical formula given that the molar mass is 275 g/mol, we need to determine the molecular mass of the empirical formula and divide it into the molar mass to obtain a whole-number multiple.
• The molecular mass of Na2SO4 is approximately (2 x 22.99) + (1 x 32.06) + (4 x 16) = 142.04 g/mol.
• Dividing the molar mass by this value gives us approximately 1.94.
• Therefore, multiplying each subscript in the empirical formula by this factor gives us a molecular formula of Na3S2O12 with a molar mass close to but not exactly equal to our given value due to rounding errors in our calculations

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