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# Empirical Formula & Products

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A compound of bromine and fluorine is used to make UF6, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37% by mass of bromine. Determine its empirical formula.

A) BrF
B) BrF2
C) Br2F3
D) Br3F
E) BrF3

Magnesium reacts with iron(III) chloride to from magnesium chloride(which can be used in fireproofing wood and in disinfectants) and iron.

3Mg(s) + 2FeCl3 à 3MgCl2 + 2Fe(s)
A mixture of 41.0 g of magnesium(molar mass =24.31 g/mol) and 175 g of iron(III) chloride (molar mass=162.2 g/mol) is allowed to react. What mass of magnesium chloride(molar mass =95.21 g/mol)
is formed?

a) 68.5 g MgCl2
b) 77.0 g MgCl2
c) 71.4 g MgCl2
d) 107 g MgCl2
e) 154 g MgCl2

https://brainmass.com/chemistry/physical-chemistry/empirical-formula-products-98763

#### Solution Summary

Handwritten answers show how to find empirical formula and products formed for 2 multiple choice questions.

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## Mole, Empirical and Stoichiometry Calculations

1. Calculate the mass of carbon in a diamond that contains 3.33 x 1024 atoms of C.
2. Calculate the mass of chloroform that contains 1,000,000,000,000 molecules of CHCL3.
3. Calculate the number of NaCL formula units in 1.37 g of table salt.
4. Calculate the number of N2 molecules in 0.111 g of nitrogen gas.

Empirical Formula Calculations (Compounds):
5. A 0.750 g sample of tin metal reacts with o.201 g of oxygen gas to form tin oxide.Calculate the empirical formula of tin Oxide.
6. A 0.565 g sample of cobalt metal reacts with excess sulfur to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product.
7. A 1.164-g sample of iron filings reacts with chlorine gas to give 3.384 g of iron chloride. Calculate the empirical formula of the product?
8. A 0.626 g sample of copper oxide was reduced to 0.500 g of copper metal by heating in a stream of hydrogen gas. Calculate the empirical formula of the copper oxide.

Stoichiometry Calculations (Precipitating Calcium Phosphate) :
9. A 0.914-g sample of stannous fluoride gives a 1.078-g precipitate of stannous phosphate. Calculate the theoretical yield and percent yield of Sn3(Po4)2.
10. A 10.000-g sample of toothpaste containing stannous fluoride gives a 0.145-g precipitate of stannous phosphate. What is the percentage of SnF2 in the toothpaste sample?

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