# What is the percentage of iron in an iron ore that is 60.0% by mass iron(III) oxide?

## Question:

What is the percentage of iron in an iron ore that is 60.0% by mass iron(III) oxide?

## The processing of iron ores:

Iron ore is majorly distributed by iron-bearing minerals such as oxides and has haematite {eq}Fe_2O_3 {/eq} as the chief ore. It, therefore, explains the relationship between the percentage mass of iron from the ore, which can be mathematically calculated using moles and molar mass of the primary ore.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerGiven data;

Percentage of iron in iron ore = 60.0% by mass of iron (iii) oxide

So let the mass of the iron ore be X

The mass of {eq}Fe_2O_3 {/eq}...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 28 / Lesson 23Read about iron, represented by the symbol Fe. Learn where iron comes from, what iron ore looks like, how iron is mined, and what iron ore is used for.

#### Related to this Question

- What is the percent composition of iron in Fe2O3?
- What mass of iron could be obtained from 40.0 g of iron (III) oxide ore which is only 75.00% pure ferric oxide?
- What is the mass of iron (g) produced from 227.4 of iron(III) oxide?
- For every 100 pounds of iron ore, there are 27.8 pounds of magnetite, Fe3O4. What is the weight percent iron in this ore? a. 72.3% b. 20.1% c. 27.8% d. 16.7% e. 23.1%
- What mass of iron can be obtained from 108g of iron (III) oxide?
- What mass of iron(III) oxide contains 52.6 grams of iron? Iron(III) oxide is 69.94% iron by mass.
- Calculate the percentage of iron in hematite ore containing 60.5 percent Fe_2O_3 by mass. How many pounds of iron would be contained in 1.00 ton of the ore?
- What mass (in grams) of iron(III) oxide contains 59.7 grams of iron? Iron(III) oxide is 69.94% iron by mass.
- What mass (in grams) of iron (III) oxide contains 45.4 g of iron?
- Iron is mined from the earth as iron ore. Calculate the mass percent composition of iron in Fe3O4 (magnetite).
- What percent by mass of iron(II) phosphate is iron?
- Iron ore contains 38% Fe_2O_3 by mass. What is the maximum amount of iron that can be extracted from 10.0 kg of this ore?
- A sample of hematite Fe_2O_3 has the mass 4.83 times 10^3 kg. a. How much iron (kg) can be extracted from this sample of hematite? b. What is the percentage of iron in this ore?
- Calculate the mass percent composition of iron for each iron ore. 1. Fe_2O_3: hematite, 2. Fe_3O_4: magnetite, 3. FeCO_3: siderite.
- Iron is mined from the earth as iron ore. Calculate the mass percent composition of iron in FeCO3 (siderite).
- Calculate the mass percent composition of iron for the second one of these iron ores: Fe2O3, Fe3O4
- Iron is mined from the earth as iron ore. Calculate the mass percent composition of iron in Fe2O3 (hematite).
- An ore was found to contain 36.0% Fe2O3 (ferric oxide) and no other iron. What mass of iron can be obtained from 36.0 grams of this ore?
- An iron ore contains 38% Fe2O3 by mass. What is the maximum mass, in kg, of iron that can be recovered from 10.0 kg of this ore?
- Iron ore is 36.0% FeO by mass. How many grams of Fe are contained in 875 grams of ore?
- How many grams of iron can be obtained from a 268 g sample of iron (III) oxide (Fe2O3)?
- 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 Fe_2O_3. The mass of Fe_2O_3 is measured to be 10.1 grams. What was the percent iron in the sample of ore?
- Calculate the formula mass of iron (lll) oxide.
- If 0.4941 g of an iron-containing compound yielded 0.1116 g of Fe_2O_3 upon oxidation, what is the mass percent of iron in the compound?
- What is the mass of 4.75 mol of the element iron (Fe)?
- Iron ore is 36.0% FeO by mass. How many grams of FeO are contained in 875 grams of ore?
- Find out which sample of iron ore contains the highest iron content by calculating the mass percentage of iron in hematite (Fe_{2}O_{3}), magnetite (Fe_{3}O_{4}), and siderite (FeCO_{3}).
- Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe2O3 (hematite), Fe3O4 (magnetite), FeCO3 (siderite).
- Determine the mass of iron in 79.2 g of Fe_2O_3.
- Hematite is an iron oxide that contains 69.9 mass % iron. Determine the empirical formula for this iron oxide.
- What is the percent by mass of oxygen in magnesium oxide, MgO?
- Two iron ores that have been used as sources of iron are magnetite (Fe3O4) and hematite (Fe2O3). Which one contains the higher mass percentage of iron?
- A sample of an impure ore contains 42.7% Cr2O3 by mass. What is the mass percentage of chromium in the ore?
- What is the mass percent of oxygen in iron(II) oxide?
- A sample of an impure ore contains 42.7% Cr_2O_3 by mass. What is the mass percentage of chromium in the ore?
- Answer the following questions about Fe(NO_3)_3. a. What is the mass percent of iron in this compound? b. A different iron compound is 34.43% by mass iron. What mass of this compound is needed to get
- How many grams of oxygen are combined with 75 g of iron to make the iron(II) oxide compound?
- A sample of iron ore contains 1.02 x 10^24 Fe atoms and is found to be 69.94% Fe by mass. What is the mass of the sample?
- What is the mass of 3.50 mol of FeCl2?
- An iron ore sample is found to be 35.00% Fe by mass. How many grams of ore are needed to obtain 454.0 grams of Fe? A. 1297 grams B. 158.9 grams C. 295.1 grams D. 350.0 grams E. none of the above
- The atomic mass of iron oxide is 160 atomic mass units. What is the atomic mass of iron, if a molecule of iron oxide consists of tow atoms of iron and three atoms of oxygen?
- A mixture of Fe_2O_3 and FeO was found to contain 72.00% Fe by mass. What is the mass of Fe_2O_3 in 0.750 g of this mixture?
- Iron ore contains 50.0% Fe2O3. How many grams of pure iron can be obtained from 200 grams of this ore?
- Calculate the mass percent composition of iron in FeO.
- What mass of iron is contained in 86.6 grams of chalcopyrite, CuFeS2?
- What mass of iron contains 6.12 times 10^{22} atoms of Fe?
- What would be the effect on the percent by mass of iron (whether it would be higher, lower, or unchanged from what it should be) calculated to be in the unknown sample and why if the sample contained
- How much iron (Fe) can be recovered from 25.0 grams of Fe2O3?
- Weight of oxygen in Fe_2O_3 and FeO in the simple ratio for the fixed amount of iron?
- An oxide of iron is found to be 77.75 \% iron by mass. Determine the empirical formula for this compound and name it.
- Suppose 2.0 grams of an oxide of iron contains approximately 0.60 grams of oxygen and 1.4 grams of iron. What is the empirical formula of the oxide?
- Calculate the mass of 500 atoms of iron (Fe).
- A piece of iron weighs 85.690 g was burned in air. The mass of the iron oxide produced was 118.350 g. a. What are the moles of iron in the original sample? b. What is the mass of oxygen in the iron oxide? c. What are the moles of oxygen in the iron oxide?
- A 70g sample of iron ore (Fe_2O_3) was analyzed for Iron and found to contain 1700 Fe. Calculate the percentage of iron in the sample.
- An iron ore was found to contain 92.0% pyrite (fool's gold). Pyrite has the formula FeS2 and is 46.5% iron. How many grams of iron are there in 65.8 grams of iron ore?
- What is the percentage of Fe in iron(II) ammonium sulfate hexahydrate, Fe(NH4)2(SO4)2 H2O?
- Calculate the mass of iron in 360 pounds of Fe3 O4.
- After 3.0 x 104 kg of an ore that contains 0.049% ilmenite is mined, the percent yield from extracting and refining the metals from the mineral is 87% for the iron and 63% for the titanium. a. Calculate the mass of iron produced from the ore. b. Calculate
- How many kilograms of red iron oxide can be obtained from 1.00 kg ferrous sulfate heptahydrate?
- The rock in a particular iron ore deposit contains 78% Fe2O3 by mass. How many kilograms of the rock must a mining company process to obtain 1.0*10^3 kg of iron?
- When 6.25 grams of pure iron are allowed to react with oxygen, a black oxide forms. If the products weighs 8.15 g, what is empirical formula of the oxide?
- What is the mass of 1.08 x 1020 atoms of iron?
- A rock is 9.4% by mass fayalite (Fe2SiO4), 6.6% by mass forsterite (Mg2SiO4), and the remainder is silicon dioxide. What is the mass percent of each element in the rock? a) Fe b) Mg c) Si and d) O
- What mass of iron is contained in 86.6 grams of FeSO_4?
- If 5.47% of a 42.2-gram sample is iron, what is the mass of the iron?
- A 33.8 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe_2O_3. The mass of Fe_2O_3 is measured to be 20.7 g. What was the mass of iron in the sample of ore?
- A 44.1 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.2 g. What was the mass of iron in the sample of ore?
- A sample of an iron oxide weighing 14.8 g is heated in a stream of H2 until it has completely converted to iron. If the iron produced has a mass of 10.36 g, THE PERCENTAGE BY WEIGHT OF OXYGEN in the original oxide must have been [{Blank}].
- An iron ore is found to contain 9.24% hematite (a compound that contains iron). (a) How many tons of this ore would contain 5.79 tons of hematite? (b) How many kilograms of this ore would contain 6.40 kg of hematite?
- The percent composition of vanadium oxide is 68.0% V and 32.0% O. Calculate the empirical formula?
- If 86.3% of the iron can be recovered from an ore that is 43.2% magnetic iron oxide, Fe3O4, what mass of iron could be recovered from 2.50 kg of this ore? The reduction of magnetic iron oxide is a complex process that can be represented in a simplified fo
- Suppose 11.89 g of iron is place in a stream of oxygen and completely reacts to give 16.99 g of the metal oxide. What would be the empirical formula for the metal oxide produce?
- What is the empirical formula of a mineral whose percent composition is 34.3% Fe, 46.0% As, and 19.7% S?
- A mixture of Fe2O3 and CuO weighing 1.000 g is reduced in a stream of hot hydrogen gas. The resulting mixture of metallic iron and metallic copper weighs 0.721 g. What was the percentage by mass of Fe2O3 in the original mixture?
- The mass of a single iron atom is 9.28E-23 grams. How many iron atoms would there be in 77.0 milligrams of iron?
- Calculate the percentage by mass of each element present in magnesium oxide, MgO.
- What is the formula of radium oxide? What is the mass percentage of radium in this oxide?
- A certain metal, M, forms two oxides, M2O and MO. If the percent by mass of M in M2O is 73.4%, what is its percent by mass in MO?
- Calculate the molar mass of Fe2O3.
- The mass of a single iron atom is 9.28 times 10^{-23} grams. How many iron atoms would there be in 162 milligrams of iron?
- The percent composition of vanadium oxide is 68% V and 32% O, Find the empirical formula?
- Calculate the mass of iron in 2.50 g of ferric nitrate non-ahydrate Fe(NO3)3 9H2O.
- After 3.0 x 104 kg of an ore that contains 0.053% ilmenite is mined, the percent yield from extracting and refining the metals from the mineral is 87% for the iron and 63% for the titanium. Calculate the mass of iron and titanium produced from the ore.
- Determine the empirical formula of a compound of a mineral having a percent composition of 29.27 percent O, 24.80 percent Fe, and 45.93 percent Cr. Assuming a 100.0 g sample of the mineral, how many grams are made up of oxygen, iron, and chromium, respect
- Wrought iron contains carbon up to what percentage?
- What is the mass in grams of 125 iron atoms?
- An oxide of vanadium is 43.99% oxygen by mass. What is the empirical formula of this oxide? A. VO2 B. VO3 C. V2O3 D. V2O5
- What is the mass, in grams, of 1.50 M of iron (iii) sulfate?
- What is the mass percent of oxygen in manganese(IV) oxide?
- If a 5.67 g block of iron metal was left to rust (i.e. react with oxygen to form iron (III) oxide), and the final block had a mass of 6.98 g, what mass of rust was formed?
- A binary compound contains only iron and oxygen. The percent, by weight, of iron is 72.360%. What is the empirical formula of the compound?
- What is the percentage by mass of oxygen in aluminum nitrate?
- Iron (III) oxide, Fe2O3, or rust is formed when iron is oxidized. How many grams of rust will be formed from the complete oxidation of 28 grams of iron? (Atomic mass of iron is 56 u and atomic mass of oxygen is 16 u). a) 80 g b) 40 g c) 56 g d) 160 g e) 3
- What is the percentage of sulfur (by mass) in SO2?
- What mass of iron contains the same number of atoms as 70.05 g of nitrogen?
- Calculate the percent by mass of the element listed first in the formula for tin(IV) oxide, SnO2.
- What is the mass in grams of 150 \times 10^{12} iron atoms, each having a mass of 56 amu?
- What is the mass in grams of 9.00 x 10^14 iron atoms, each having a mass of 56 amu?
- What is the mass number of an iron atom with 28 neutrons?
- A 0.020 M K M n O 4 solution was used to determine the percent iron in a sample containing iron(II according to the equation M n O 4 + 5 F e 2 + + 8 H + M n 2 + + 5 F e 3 + + 4 H 2 O . It took 25.0 mL of the K M n O 4 to completely react with al