a piece of nickel foil has dimensions of 1.250 cm x 1.250 x 0.5500cm. it reacts with fluorine gas to produce 1.261 grams of compound. the density of nickel is 8.908 g/cm^3
a.)what is the empirical formula?
can you show me how you got to this answer too, thanks sooo much!!! :)
a.)what is the empirical formula?
can you show me how you got to this answer too, thanks sooo much!!! :)
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The size of the nickel foil will give you the volume
Using the the density you will get you the mass of the metal
volume= 1.250 x 1.250 x 0.05500 = 0.08594 cm^3
the density is 8.908 g / cm^3 so the mass = 0.08594 x 8.908 = .76553 g
moles of Ni = .76553 / 58.69 = .0130 moles
mass of F = 1.261 - .76553 = 0.49547 g or .49547 / 19 =
0.0261 moles of F
molar ratio of Ni : F = 1:2
empirical formula is NiF2
Using the the density you will get you the mass of the metal
volume= 1.250 x 1.250 x 0.05500 = 0.08594 cm^3
the density is 8.908 g / cm^3 so the mass = 0.08594 x 8.908 = .76553 g
moles of Ni = .76553 / 58.69 = .0130 moles
mass of F = 1.261 - .76553 = 0.49547 g or .49547 / 19 =
0.0261 moles of F
molar ratio of Ni : F = 1:2
empirical formula is NiF2