Jul 23, 2012· A 35.2 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 17.3 g. What was the mass of iron in the sample of ore? Answer in units of g

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) what is the theoretical yield of iron? asked by Kim on March 28, 2010; Analytical chemistry. 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.

Iron ores are rocks and minerals from which metallic iron can be economically extracted. The ores are usually rich in iron oxides and vary in color from dark grey, bright yellow, or deep purple to rusty red. The iron is usually found in the form of magnetite (Fe 3 O 4, 72.4% Fe), hematite (Fe 2 O 3, 69.9% Fe), goethite (FeO(OH), 62.9% Fe), limonite (FeO(OH)·n(H 2 O), 55% Fe) or siderite (FeCO ...

A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction:Fe2O3 (s) + 3 C (s) → 2 Fe (s) + 3 CO (g)What is the mass percent of Fe 2O3 in the impure iron ore sample? Assume that Fe 2O3 is the only source of iron and that the reaction is …

Magnetite, an iron ore with formula Fe3O4, can be reduced by treatment with hydrogen to yield iron metal and water vapor. (a) Write the balanced equation. (Use the lowest possible coefficients.) 1Fe3O4(s) + 4H2(g)-> 3Fe(s)...

The charts give an overview on major current developments in global mining production based on World Mining Data 2018. Ratio of Iron Ore to all other Ferro-Alloy Metals is 97.6 % to 2.4 % Growth rate of total Iron Ore production 2000/2016 is 162.0 % 4 countries share more than 80 %. Other 10.4% Ukraine 2.6% South Africa 2.7% Russia 3.5% India 7 ...

2004 B (repeated in thermodynamics) 2 Fe (s) + 3 2 O 2(g) Fe 2 O 3(s) ∆H f˚ = -824 kJ mol–1 Iron reacts with oxygen to produce iron(III) oxide as represented above. A 75.0 g sample of Fe (s) is mixed with 11.5 L of O 2(g) at 2.66 atm and 298 K. (a) Calculate the number of moles of each of the following before the reaction occurs.

Sep 06, 2013· -if a 1,52g sample yields Mn3O4 weighing 0.126g (a)what will be percent Mn2O3 in sample? (B)what is the percent of Mn? 2. A mixture containing only FeCl3 and AlCl3 weighs 5,95g. The chlorides are converted to the hydrous oxide and ignited to Fe2O3 and Al2O3. The oxide mixture weighs 2,62g. Calculate the percent of Fe and Al in the original mixture.

Solution for a sample of 0.2952 g iron ore is dissolved in acid, and the iron is converted to Fe2+. the sample is then titrated with 47.20 ml of 0.02240 M KMnO4…

Oct 15, 2019· Show your work. (a) 150.0 g of Fe2O3 (b) 2.50 x 1021 molecules of ethanol, C2H,OH 2. Iron oxide ore, Fe,O4 yield elemental iron when heated to a very high temperature with carbon monoxide. The equation for the chemical process is Fe(s) CO2(g) Fe2O3(s) CO(g) (a) Balance the chemical equation.

Arial Franklin Gothic Book Perpetua Wingdings 2 Calibri Equity 1_Equity 2_Equity 3_Equity 4_Equity A 100-gram sample of iron ore was found to contain 44 grams of iron. How many grams of iron are in a 450-gram sample of the ore The density of a liquid is 0.821 g/mL.

Jul 12, 2020· 0.7 g sample of iron ore was dissolved in acid. Iron was reduced to `+2` state and it required 50 " mL of " `(M)/(50)` `KMnO_(4)` solution for titration. The percentage of …

Jul 11, 2010· Assume a 100-g sample of each ore. Convert that amount to moles by dividing by the ore's respective molecular weight, and then take the ratio of iron in the ore, and the ore itself. Then multiply by the molecular weight of iron to find the weight of iron in that 100 g sample. The mass percent would be massFe / massSample * .

•Example -A 335 g sample of ore yields 29.5 g of iron. What is the percent of iron in the ore? 46 Percentage • Percentage is the parts per hundred of a sample. • Example -A 335 g sample of ore yields 29.5 g of iron. What is the percent of iron in the ore? 8.81% x 335 g ore 29.5 g Fe x

For the following reaction, 4.80 grams of oxygen gas are mixed with excess iron . The reaction yields 18.4 grams of iron(II) oxide . iron ( s ) + oxygen ( g ) iron(II) oxide ( s )

Aug 19, 2016· Approx. 15*g of metal. "Moles of iron oxide, " Fe_2O_3 = (21.6*g)/(159.69*g*mol) = 0.135*mol with respect to the oxide. But by the composition of the oxide, there are thus 2xx0.135*molxx55.8*g*mol^-1 "iron metal" = ??g. An extraordinary percentage of our budgets goes into rust prevention; "iron(III) oxide" is only part of the redox chemistry. Once you put up a bridge or a …

A 1.362 g sample of an iron ore that contained Fe3O4 was dissolved in acid with all of the iron being reduced to iron (II). The solution was acidified with sulfuric acid and titrated with 39.42 mL of 0.0281 M KMnO4, which oxidized the iron (II) to iron (III) while reducing the permanganate to manganese (II).

Aug 01, 2020· Solution for a sample of 0.2952 g iron ore is dissolved in acid, and the iron is converted to Fe2+. the sample is then titrated with 47.20 ml of 0.02240 M KMnO4…

A 500.0 g iron ore sample was determined to contain 242 g of iron. What is the mass percent of iron in the ore? 48.4. ... If a canister absorbed 225.0 g of CO2 from the air that resulted in the production of 66.30 g of H2O, what was the percent yield of Li2CO3? 71.96%.

Sep 10, 2018· For the iron ore concentrate, the GBT-10322.1-2000 standard stipulates we can use the auger sampling system to sample unless the auger sampler can reach the bottom of the iron ore storage and the auger hopper which is filled with iron ore. TOP-SAMPLER promises that our all sampling systems can meet this requirement and the sampling procedure is random and effective.

A 47.5 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 7.3 grams.

Feb 05, 2008· The amount of iron in ore can be quantitatively determined by titrating a solution of the unknown with a standard solution of potassium dichromate. The reaction that occurs is 6Fe^2+(aq) + Cr2O7^2-(aq) + 12H^+(aq) ---> 6Fe^3+(aq)+2Cr^3+(aq)+7H2O(aq) A. The titration of 25.0 ml of an iron(II) solution required 18.0 ml of a 0.125 M solution of potassium dichromate to reach the …

0. 8 0 4 g sample of iron ore was dissolved in acid. Iron was oxidised to + 2 state and it required 4 7 . 2 mL of 0 . 1 1 2 N K M n O 4 solution for titration. If the percentage of

Aug 01, 2020· `0.804 g` sample of iron ore was dissolved in acid. Iron was oxidised to `+2` state and it requires `47.2 mL` of `0.112N KMnO_(4)` solution for titration, Calculate `%` of `Fe` and `Fe_(3)O_(4 ...

A 818-g sample of impure iron ore is heated with excess carbon, producing 296 g of pure iron by the following reaction: Fe2O3(s) + 3C(s) + 2Fe + 3 CO(g) What is the mass percent of Fe2O3 in the impure iron ore sample? Assume that is the only source of iron and that the reaction is efficient.

Stoichiometry is the chemistry that mathematically relates all substances in a reaction, quantitatively relating the amount of reactants and products in a chemical reaction. It allows the chemist to determine the amount of product that will form from a given amount of reactants, or the amount of one reactant that is needed to react completely with some specific amount of the other reactant.

Mining companies use this reaction to obtain iron from iron ore: fe2o3 (s) + 3 co (g) →2 fe (s) + 3 co2 (g) the An ore contains fe3o4 and no other iron. the iron in a 51.9-gram sample of the ore …

Answer to: 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...

In production of iron (Fe) for use in iron and steel industries, Iron (III) oxide (Fe₂O₃) is a very important mineral ore (hematite). Iron (III) oxide is used in many industrial reactions such as carbothermal reduction to produce iron.-----The mass of FeO3 in the iron ore will be: 90% of the 100kg ore 90/100 × 100 = 90 kg of Fe₂O₃