In: Chemistry
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 (SnxOy) of the original oxide of tin?
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 (SnxOy) 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