A sample of an oxide of vanadium weighing 4.589 g was reduced with hydrogen gas to form water and another oxide of vanadium weighing 3.782 g. The second oxide was reduced further with hydrogen gas until only 2.573 g of vanadium metal remained. a. Calculate the empirical formulas of the two oxides?

Q: What is the mass percent of iron in iron(II) phosphide

A: Fe2P Molar mass of Fe2P=142.66gm/mole Atomic mass of Fe = 55.85gm/mole

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A: 1 mole of vanadium contains Avogadro’s number of atoms. The number of mole of 1.28 g of vanadium…

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Q: (V,Os) (1.0 × 10º)- Calculate the mass of vanadium(V) oxide that contains a million vanadium atoms.

A: Given : number of V atoms = 1.0 × 106 atoms  To calculate :- mass of V2O5

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A: Mass = Volume x density Number of moles = Mass/molar mass Number of molecules = 6.0224 x 1023 x…

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Q: 6. Give the empirical formula for the following compounds: b)_

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A: atomic mass is mass of atom which have amu unit .

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Q: titanium

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A: Calculate the percent by mass of each component present in the alloy sample.

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Q: the mass percent of magnesium in MgSO4.

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Mass Spectrometry

This process is an instrumental method in which a sample is changed to fast moving positive ions by electron bombardment. The charged particles vary due to their different mass to charge ratio and are estimated with the help of this difference. It is also called mass spectroscopy.