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6,96 g of nitric oxide are obtained.
Aluminum oxide, Al2O3 would produce aluminum by the following decomposition:2Al2O3 ==> 4Al + 3O2 750.0 g Al2O3 x 1 mole/101.96 g = 7.356 moles Al2O3 Theoretical yield of Al = 7.356 moles Al2O3 x 4 moles Al/2 mole Al2O3 = 14.71 moles Al Theoretical mass of Al = 14.71 moles Al x 26.98 g/mole = 396.9 g Al Percent yield = 256.734 g/396.9 g (x100%) = 64.68% yield (to 4 significant figures)
Yes, it is correct; a thermite reaction.
Yes, it is correct. A thermite reaction.
Nitrogen oxide is formed after reaction with ozone. It is also an ozone depleting substance.
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whatis the word equation of Iron oxide when metal oxide is added and what gas is produced in the reaction
The mass of nitrous oxide is 262,8 g.
A theoretical yield is equivalent to a percent yield of 100. In practice, it is very rare to achieve 100 yield from a reaction due to a wide range of outside factors 1.7mol
6,96 g of nitric oxide are obtained.
26.20
copper , nitrogen & water produced
The actual yield is 73 %.
In the presence of oxygen a reaction occur (oxidation) and the hydrated iron oxide is produced.
33.0%
The percent yield in this case is 89,25 %.
Aluminum oxide, Al2O3 would produce aluminum by the following decomposition:2Al2O3 ==> 4Al + 3O2 750.0 g Al2O3 x 1 mole/101.96 g = 7.356 moles Al2O3 Theoretical yield of Al = 7.356 moles Al2O3 x 4 moles Al/2 mole Al2O3 = 14.71 moles Al Theoretical mass of Al = 14.71 moles Al x 26.98 g/mole = 396.9 g Al Percent yield = 256.734 g/396.9 g (x100%) = 64.68% yield (to 4 significant figures)