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

A 2.540 g 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.

a) What is the mass percent of tin in SnO₂?

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

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

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

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

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

g) What is the formula (Sn_xO_y) of the original oxide of tin?

Solutions

Expert Solution

a) What is the mass percent of tin in SnO₂?

Mass percent of Sn = (Atomic mass of Sn/Molar mass of SnO2)*100

mass% of Sn = (118.71/150.71)*100 = 78.76%

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

Mass of Sn = (Atomic mass of Sn/Molar mass of SnO2)*Mass of sample

mass of Sn = (118.71/150.71)*2.842 = 2.238 g

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

mass of Sn = (118.71/150.71)*2.540 = 2.00 g

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

mass of O = (2*16.0/150.71)*2.54 = 0.54 g

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

No. of moles of Sn = Mass of Sn/ Atomic mass = 2.00g/118.71g/mo/ = 0.0168 moles

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

No. of moles of O = Mass of O/ Atomic mass = 0.54g/16 g/mo/ = 0.0337 moles

g) What is the formula (Sn_xO_y) of the original oxide of tin?

To get simple ratio, divide the moles of Sn and O with smallest number 0.0168

0.0168/0.0168 = 1 and 0.0337/0.0168 = 2

Formula of Tin oxide is SnO2

queen_honey_blossom answered 1 year ago

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