a 0.279g sample of iron was heated to the resulting product with a mass of 0.400g...

Question

Question

a 0.279g sample of iron was heated to the resulting product with a mass of 0.400g determine the empirical formula for the compound

Answer 1

Answer #1

Molar mass of Fe 56 g/mole Thus, moles of Fe in 0.279 g of it mass/molar mass 0.005 mass of O in the formed oxide 0.4 -0.279

Answer 2

Similar Homework Help Questions

A 21.92 gram sample of iron is heated in the presence of excess oxygen. A metal...

A 21.92 gram sample of iron is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 31.33 g. Determine the empirical formula of the metal oxide. A 25.23 gram sample of chromium is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 43.67 g. Determine the empirical formula of the metal fluoride. A 7.199 gram sample of iron is heated in the presence of excess bromine....
A 18.47 gram sample of iron is heated in the presence of excess iodine. A metal...

A 18.47 gram sample of iron is heated in the presence of excess iodine. A metal iodide is formed with a mass of 102.4 g. Determine the empirical formula of the metal iodide. Enter the elements in the order Fe, I empirical formula = A 10.44 gram sample of cobalt is heated in the presence of excess bromine. A metal bromide is formed with a mass of 38.74 g. Determine the empirical formula of the metal bromide. Enter the elements...
A 7.143 gram sample of iron is heated in the presence of excess iodine. A metal...

A 7.143 gram sample of iron is heated in the presence of excess iodine. A metal iodide is formed with a mass of 55.83 g. Determine the empirical formula of the metal iodide. Enter the elements in the order Fe, I empirical formula =

A sample of an oxide of iron was found to contain 72.34% by mass of iron and 27.66% by mass of oxygen. What is the empir...

A sample of an oxide of iron was found to contain 72.34% by mass of iron and 27.66% by mass of oxygen. What is the empirical formula for this compound? (The correct answer is Fe3O4, but I’m not sure how to do the math)
A iron carbonyl compound is heated to release CO and leave elemental iron behind. Treatment of...

A iron carbonyl compound is heated to release CO and leave elemental iron behind. Treatment of 6.544 g of the compound releases 2.085 L of CO(g) at 25.00 °C and 1.960 atm pressure. Determine the empirical formula of this compound. Given that its molar mass is 195.90, choose its structural formula from the metal carbonyls shown below, where M = Fe. Pick one of the below. Occo co Oc—MAMco oc' do co 1000000 00 -00 05 06 0000 occo OCCO...
A sample of scandium metal weighing 8.565 g is heated in air and combines with oxygen....

A sample of scandium metal weighing 8.565 g is heated in air and combines with oxygen. The resulting compound weighs 13.137 g. Calculate the following: a. Mass of oxygen reacted? b. Moles of scandium atoms? c. Moles of oxygen atoms? d. The empirical formula of the compound?

A 17.59 gram sample of copper is heated in the presence of excess bromine. A metal...

A 17.59 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 39.71 g. Determine the empirical formula of the metal bromide. Enter the elements in the order Cu, Br empirical formula= A 10.70 gram sample of chromium is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 22.42 g. Determine the empirical formula of the metal fluoride. Enter the elements in...
-- 0 02 -.UJU U CILJI UUUU. 26. A 3.78 g sample of iron metal is...

-- 0 02 -.UJU U CILJI UUUU. 26. A 3.78 g sample of iron metal is reacted completely with sulfur to produce 5.95 g of iron sulfide. Determine the empirical formula and enpirical formula mass of this compound.
A 13.56 gram sample of copper is heated in the presence of excess bromine. A metal...

A 13.56 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 30.60 g Determine the empirical formula of the metal bromide. ter the elements in the order C B empirical formula A 5.267 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 13.29 grams of CO2 and 2.332 grams of H20 are produced In a separate experiment, the molar mass...

4) Hypothetical Data for Analysis An oxide of iron is 69.94% iron by mass. Calculate its...

4) Hypothetical Data for Analysis An oxide of iron is 69.94% iron by mass. Calculate its empirical formula and determine the name of the ionic compound. (Hint: assume you have a 100 g sample of the oxide of iron. How many grams would be iron? Then how many grams would be oxygen? Convert those to moles. Find the ratio. Find the nearest whole number ratio). Then determine its name.