Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Elements
Iron ore analysis
A 70g sample of iron ore(Fe2O3) was analyzed for Iron and found to contain 1700 Fe. Calculate the percentage of iron in the sample.
1 answer
how much iron in the sample?
percentage=IRONinSample/70 * 100
You can
ask a new question
or
answer this question
.
Similar Questions
A 25.2 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
Mass Fe in sample = (12 x 2 x atomic mass Fe/molar mass Fe2O3) = ? %Fe = (mass Fe/mass sample)*100 =
Read more.
A 44.6 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
What fraction, F, of the mass of a Fe2O3 molecule is FE ? total mass of molecule = 2(atomic mass
Read more.
A 46.9 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
Convert 11.6 g Fe2O3 to g Fe. The easy way to do that is to multiply by a chemical factor which,
Read more.
A 40.3 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
Isn't this done the same as the problems before? Try it yourself first.
Read more.
A 39 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
mols Fe2O = grams/molar mass = ? mols Fe = twice that since there are two mols Fe in each mole of
Read more.
A 28.6 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
Same song, fifth dance.
Read more.
A 36.5 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
Indicate your subject in the "School Subject" box, so those with expertise in the area will respond
Read more.
A 37.2 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
Top answer:
To find the percent of iron in the sample of ore, we need to calculate the mass percent. First,
Read more.
A 7.6 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a series of chemical reactions to
Top answer:
Didn't I do this for you (or one similar to it) a couple of days ago. 12.9g x (1 mol Fe2O3/molar
Read more.
A 7.7 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a series of chemical reactions to
Top answer:
You end up with 25.4 g Fe2O3. 25.4g Fe2O3 x (2*atomic mass Fe/molar mass Fe2O3) = mass Fe. Piecemeal
Read more.
Related Questions
the balanced equation for the reduction of iron ore to the metal using CO is Fe2O3+3CO(g) -> 2Fe+3CO so what is the maximum of
When 84.8 g of iron(III) oxide reacts with an excess of carbon monoxide, iron is produced.
Fe2O3(s) + 3CO(g) ==> 2Fe(s) + 3CO2(g)
The iron in a 0.6656 g ore sample was reduced quantitatively to the +2 state and then titrated with 26.753 g of KMnO4 solution.
An iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe2+(aq). The iron solution was titrated with
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide.
A 0.5962g sample of iron ore is dissolved in acid producing Fe3+. Through a series of reactions, the iron precipitates as the
(Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are
Iron is found in Earths crust as several different iron compounds. Calculate the mass (in kg) of each compound that contains 1.0
The rock in a particular iron ore deposit contains 84 % Fe2O3 by mass.
How many kilograms of the rock must be processed to obtain
The rusting of iron is represented by the equation 4Fe +3O2 --> 2Fe2O3. If you have a 1.50-mol sample of iron, how many moles of