Question

In: Chemistry

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 (SnxOy) 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 (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


Related Solutions

A 0.500 g sample containing Ag2O and inert material is heated, causing the silver oxide to...
A 0.500 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C. a.) 25.1% b.) 51.9% c.)12.5% d.) 50.1%
A sample of 58.90 g solid benzene at −2.3°C was heated until it absorbed 13.2 kJ...
A sample of 58.90 g solid benzene at −2.3°C was heated until it absorbed 13.2 kJ of heat, at a constant pressure of 1 atmosphere. Using the data given in the table below, determine the final phase and final temperature of the benzene sample. Properties of Benzene Values melting point 5.49°C boiling point 80.09°C heat of fusion at 5.49°C 9.87 kJ/mol heat of vaporization at 80.09°C 30.72 kJ/mol molar heat capacity of solid at 0°C 118.4 J/mol·K molar heat capacity...
A 1.250 g sample of barium chloride hydrate, BaCl2.xH2O, was heated until all the water had...
A 1.250 g sample of barium chloride hydrate, BaCl2.xH2O, was heated until all the water had been driven off. The remaining anhydrous salt weighed 1.060g. Use this data to calculate the value of x, the number of moles of water of crystallization in the hydrated salt. You MUST Show ALL your work for full credit! 5. 0.0185 mol of hydrated magnesium sulfate MgSO4.xH2O has a mass of 4.56g. Calculate the value of x, the number of moles of water of...
A) Water (2350 g ) is heated until it just begins to boil. If the water...
A) Water (2350 g ) is heated until it just begins to boil. If the water absorbs 5.83×105 J of heat in the process, what was the initial temperature of the water? Express your answer with the appropriate units. B) If 125 cal of heat is applied to a 60.0-g piece of copper at 22.0 ∘C , what will the final temperature be? The specific heat of copper is 0.0920 cal/(g⋅∘C) .
A. Determine the percent composition of a compound formed from 0.500g of tin reacting with oxygen and forming 0.635 g of the oxide.
  A. Determine the percent composition of a compound formed from 0.500g of tin reacting with oxygen and forming 0.635 g of the oxide. B. Determine the empirical and molecular formulas for a compound that has a molar mass of 62g/mol and is 38.7%C, 9.74%H and 51.6%O by mass. C. Determine the empirical and molecular formula for a compound that is 31.42% S, 31.35% O and 37.23%F and has a molar mass of 102.1g/mol. D. Determine the number of oxygen...
A 50 g ice cube initially at - 30 0C is heated until it has completely...
A 50 g ice cube initially at - 30 0C is heated until it has completely been changed to steam at 120 0C, how much heat energy in calories has been added? ( Specific heat of ice is 0.5 ca/g 0C and that of steam is 0.48 cal/ g 0C , that of water is 1 cal/g 0C ; Latent heat of fusion of ice is 80 cal/g, Latent haet of vaporization is 540 cal/g ).
A sample of impure limestone (calcium carbonate) when heated yields calcium oxide and oxygen gas. A...
A sample of impure limestone (calcium carbonate) when heated yields calcium oxide and oxygen gas. A 1.506 g sample of limestone gives 0.558 g of carbon dioxide. This is less than what was expected. Calculate the percent of limestone in the impure sample.
A sample of impure limestone (calcium carbonate) when heated yields calcium oxide and oxygen gas. A...
A sample of impure limestone (calcium carbonate) when heated yields calcium oxide and oxygen gas. A 1.506 g sample of limestone gives 0.558 g of carbon dioxide. This is less than what was expected. Calculate the percent of limestone in the impure sample.
If a sample of A(g) at 2.10 atm is heated to 500K, what is the pressure...
If a sample of A(g) at 2.10 atm is heated to 500K, what is the pressure of B(g) at equilibrium? 2A(g)--> B(g) Kp=8.74*10^-5 at 500 K
Analysis of a 2.016 g sample of pure magnesium oxide gave 1.216 g magnesium and 0.800...
Analysis of a 2.016 g sample of pure magnesium oxide gave 1.216 g magnesium and 0.800 g of oxygen. A second sample weighing 4.479 g was found to contain 2.701 g magnesium and 1.776 g oxygen. Show that these data are in agreement with the law of definite composition.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT