A 2.540g sample of an oxide of tin was heated in the air until the mass of the s

Question

A 2.540g sample of an oxide of tin was heated in the air until the mass of the sample no longer changed, and 2.842 g of tin (IV) oxide (SnO2) was obtained as a result of the heating.

1) What is the mass percent of tin in SO2?

2) What is the mass of tin in the final sample?

3) What was the mass of tin in the original sample?

4) What was the mass of oxygen in the original sample?

5) What was the number of moles of tin in the original sample?

6) What was the number of moles of oxygen in the original sample?

7) What is the formula (SnxOy) of the original oxide of tin?

Explanation / Answer

1) Molar mass of SnO2 = 150.71g/mol

Molar mass of Sn = 118.71g/mol

mass % of Sn in SnO2 = (118.71g/150.71g)×100 = 78.77%

2) Mass of Tin in final sample =( 78.77/100)×2.842g = 2.239g

3) Mass of Tin in original sample = 2.239g

4) Mass of oxygen in original sample = 2.540g - 2.239g = 0.301g

5) No of moles of tin in original sample = 2.239g/118.71g/mol = 0.01886

6) No of moles of oxygen = 0.301g /16g/mol = 0.01881

7) SnO

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