# 335 g sample of ore yields 29 5 g of iron

• ### ChemTeam Dilution Problems #1-10

Problem #7 To what volume should you dilute 133 mL of an 7.90 M CuCl 2 solution so that 51.5 mL of the diluted solution contains 4.49 g CuCl 2 Solution 1) Find moles (4.49g CuCl 2) (1 mole CuCl 2 / 134.45 grams) = 0.033395 moles CuCl 2. 2) Find the molarity of the 51.5 mL of the diluted solution that contains 4.49g CuCl 2 (0.033395 moles CuCl 2) / (0.0515 liters) = 0.648 M

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• ### definition mole explained molar mass mol mols calculations

(a) 8.4 g of iron was heated in air to form an oxide until there was no longer any gain in weight. The final mass of the iron oxide was 11.6 g. There was only one product of the reaction. Atomic masses Fe = 56 O = 16 (i) Calculate the mass of oxygen that combined with the iron.

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• ### How to Calculate Percent Yield in a Chemical Reaction

Theory predicts that 46.59 g of sodium sulfate product is possible if the reaction proceeds perfectly and to completion. But the question states that the actual yield is only 37.91 g of sodium sulfate. With these two pieces of information you can calculate the percent yield using the percent-yield formula

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• ### ChemTeam Dilution Problems #1-10

Problem #7 To what volume should you dilute 133 mL of an 7.90 M CuCl 2 solution so that 51.5 mL of the diluted solution contains 4.49 g CuCl 2 Solution 1) Find moles (4.49g CuCl 2) (1 mole CuCl 2 / 134.45 grams) = 0.033395 moles CuCl 2. 2) Find the molarity of the 51.5 mL of the diluted solution that contains 4.49g CuCl 2 (0.033395 moles CuCl 2) / (0.0515 liters) = 0.648 M

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• ### Energy BasicsLumen LearningSimple Book Production

How much heat in joules and in calories must be added to a 75.0–g iron block with a specific heat of 0.449 J/g °C to increase its temperature from 25 °C to its melting temperature of 1535 °C How much heat in joules and in calories is required to heat a 28.4-g (1-oz) ice cube from

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• ### ChemTeam Dilution Problems #1-10

Problem #7 To what volume should you dilute 133 mL of an 7.90 M CuCl 2 solution so that 51.5 mL of the diluted solution contains 4.49 g CuCl 2 Solution 1) Find moles (4.49g CuCl 2) (1 mole CuCl 2 / 134.45 grams) = 0.033395 moles CuCl 2. 2) Find the molarity of the 51.5 mL of the diluted solution that contains 4.49g CuCl 2 (0.033395 moles CuCl 2) / (0.0515 liters) = 0.648 M

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• ### Can some1 show me how to workout this problem Yahoo Answers

Jan 29 2011 · One of the reactions that occurs in a blast furnace where iron ore is converted to cast iron is Fe2O3 3CO 2Fe 3CO2 Suppose that 1.64 x 103 kg of Fe are obtained from a 2.62 x 103 kg sample of Fe2O3. Assuming that the reaction goes to completion what is the percent purity of Fe2O3 in the original sample My answer is 4.9 x 1o -4 .

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4. Use the following balanced equation. Calculate the theoretical yield of iron if 16.5 grams of Fe 2 O 3 are completely reacted. 2 O 3 3H 2 2Fe 3H 2 O 16.5 g x grams moles moles 16.5 g Fe2O3 1 mol Fe2O3 159.70 g Fe2O3 2 mol Fe 1 mol Fe2O3 55.85 g Fe 1 mol Fe = 11.5 g Fe 5

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• ### Experiment 16 Help uml.edu

4. Fe by Mass in Unknown Sample 1 . The percentage of iron in Unknown sample 1 represents what fraction of the total sample is Fe. Unknown Sample 1 had a total mass of 1.2352 g. We have just determined that 0.1488 g of this is Fe. So the Fe

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• ### Chapter 3. Stoichiometry Mole-Mass Relationships in

Skill 3-5 contd Vitamin C (M= 176. g/mol) contains C H and O. A 1.000 g sample was placed in a combustion apparatus Plan -Use changes in mass of CO 2 and H 2 O absorbers to calculate the moles of C and H present in the sample. -Find the mass of C using the mass fraction of C in CO 2. Likewise find the mass of H from the mass of H 2 O.

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• ### 335 g sample of ore yields 29 5 g of iron

A 335 g sample of ore yields 295 g of iron What is the percent of iron in the ore Density and Specific Gravity Density = mass/volume or D = m/V Densities may be used to distinguish between two substances or in identifying a particular substance Expressed in g/cm3 or g/mL for liquids and solids and g/L for gases Example 6 Density mass volume

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• ### GEOPHYSICAL METHODS IN EXPLORATION AND MINERAL

reflection B G Thermal bore-hole or shallow Thermal gradient or Degrees C/m degrees C Thermal conductiv- Thermal flux or con- Hole depth hole B temperature ity ductivity variations Thermal remote sensing A G Surface temperature Degrees C Thermal inertia Thermal inertia con- About 5 cm day and night trasts Electrical (see text)

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• ### What is the theoretical yield of iron(II) oxide in grams

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 )

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Crystal orientation dictated epitaxy of ultrawide-bandgap 5.4- to 8.6-eV α-(AlGa) 2 O 3 on m-plane sapphire By Riena Jinno Celesta S. Chang Takeyoshi Onuma Yongjin Cho Shao-Ting Ho Derek Rowe Michael C. Cao Kevin Lee Vladimir Protasenko Darrell G. Schlom David A. Muller Huili G. Xing Debdeep Jena

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• ### Chemistry Worksheets

9) 28.5 g of iron shot is added to a graduated cylinder containing 45.50 mL of water. The water level rises to the 49.10 mL mark From this information calculate the density of iron. 10) What volume of silver metal will weigh exactly 2500.0 g. The density of silver is 10.5 g/cm3. States of matter elements compounds mixtures

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• ### ChemTeam Calculate empirical formula when given mass data

Example #11 A 4.628-g sample of an oxide of iron was found to contain 3.348 g of iron and 1.280 g of oxygen. What is simplest formula for this compound Solution 1) Determine moles of each element iron 3.348 g / 55.845 g/mol = 0.05995 mol = 0.06 mol oxygen 1.280 g / 16.00 g/mol = 0.08 mol

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• ### Engineering Handbook

materials used in steelmaking are iron ore coal and limestone. These materials are converted in a blast furnace into a product known as "pig iron " which contains considerable amounts of carbon (above 1.5 ) manganese sulfur phosphorus and silicon. Pig iron is hard brittle and unsuitable for direct processing into wrought forms.

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• ### ChemTeam Calculate empirical formula when given mass data

Example #11 A 4.628-g sample of an oxide of iron was found to contain 3.348 g of iron and 1.280 g of oxygen. What is simplest formula for this compound Solution 1) Determine moles of each element iron 3.348 g / 55.845 g/mol = 0.05995 mol = 0.06 mol oxygen 1.280 g / 16.00 g/mol = 0.08 mol

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• ### Journal of Cleaner Production ScienceDirect by Elsevier

Information and Communication Technologies (ICT)-based Innovations for Sustainable Production and Service Operations Management. Edited by Thomas Welsh Archibald Yiwen Bian Hua Cai Yutao Wang. 9 January 2021. Innovations in Green and Blue Infrastructure in Cities Analyzing the Impacts on Natural Resources and Global Change.

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• ### ChemTeam Calculate empirical formula when given mass data

Example #11 A 4.628-g sample of an oxide of iron was found to contain 3.348 g of iron and 1.280 g of oxygen. What is simplest formula for this compound Solution 1) Determine moles of each element iron 3.348 g / 55.845 g/mol = 0.05995 mol = 0.06 mol oxygen 1.280 g / 16.00 g/mol = 0.08 mol

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• ### 10 Biggest Mining CompaniesInvestopedia

Sep 14 2020 · Below we look at the 10 biggest mining companies by 12-month trailing revenue. Some companies outside the U.S. report profits semi-annually instead of quarterly so the 12-month trailing data may

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• ### 8517China Customs HS Code China Import Tariffs for

Latest China HS Code tariff forTariff duty regulations restrictions landed cost calculator customs data for in ETCN. China customs statistics trade data.

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• ### Iron(II) sulfateWikipedia

Iron(II) sulfate (British English iron(II) sulphate) or ferrous sulfate denotes a range of salts with the formula Fe SO 4 ·xH 2 O. These compounds exist most commonly as the heptahydrate (x = 7) but are known for several values of x.The hydrated form is used medically to treat iron deficiency and also for industrial applications.

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• ### Example 1 5 A 335 g sample of ore yields 295 g of iron

This preview shows page 5778 out of 85 pages. • Example 1-5 A 335 g sample of ore yields 29.5 g of iron. Example 1-5 A 335 g sample of ore yields 29.5 g of iron. What is the percent of iron in the ore You do it

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• ### EXERCISESSTOICHIOMETRY CALCULATIONS WITH CHEMICAL

3.29 Without doing any detailed calculations 3.64 An iron ore sample contains Fe 2 O 3 together with other substances. Reaction of the ore with CO produces iron metal Fe 2 O 3 (s) Calculate the theoretical yield of C 2 H 5 Cl when 125 g of C 2 H 6 reacts with 255 g of Cl 2

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• ### How to Calculate ConcentrationThoughtCo

Sep 05 2018 · 12 g iron / 100 g sample = x g iron / 250 g sample Cross-multiply and divide x= (12 x 250) / 100 = 30 grams of iron How to Calculate Volume Percent Concentration of a Solution . Volume percent is the volume of solute per volume of solution. This unit is used when mixing together volumes of two solutions to prepare a new solution.

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• ### EXERCISESSTOICHIOMETRY CALCULATIONS WITH CHEMICAL

3.29 Without doing any detailed calculations 3.64 An iron ore sample contains Fe 2 O 3 together with other substances. Reaction of the ore with CO produces iron metal Fe 2 O 3 (s) Calculate the theoretical yield of C 2 H 5 Cl when 125 g of C 2 H 6 reacts with 255 g of Cl 2

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• ### Answers Moles and Stoichiometry Practice Problems

Calculate the mass of iron (in grams) that can be formed from this mixture of reactants. 1.75 mol Fe 2 O 3 x 2 mol Fe x 55.845 g Fe = 195 g Fe 1 mol Fe 2 O 3 1 mol Fe 5.73 g FeCl 3 169.872g AgNO 3 3 mol AgNO 3 1 mol FeCl 3 Therefore 32.4g5.73g = 26.7g FeCl 3 remains after the reaction is over.

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• ### Redox titration (calculating percent iron in sample

Apr 18 2010 · A mass of iron ore weighing 0.2792g was dissolved in dilute acid and all the iron was converted to Fe2 (aq). The iron II solution required 23.30ml of 0.0194M KMnO4 for titration. Calculate the percentage of iron in the ore. Homework Equations Wrote out my redox reactions MnO4- 8H 5e- ---> Mn2 4H2O (2) Fe ---> Fe2 2e- (5)

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• ### Iron reacts with oxygen to form iorn(III) oxide according

Apr 10 2008 · Iron reacts with oxygen to form iorn(III) oxide according to the reaction 4Fe(s) 3O2(g)---->2Fe2O3(s) If you begin with 3.46g of Fe a)what mass in grams of O2 is required for complete reaction

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• ### Worksheet #1 Stoichiometry

Calculate the theoretical yield in grams of Fe produced by the reaction of 5.67 g of iron III oxide. If the actual yield is 2.00 g calculate the percentage yield. 2Fe 2 O 3 3C → 4Fe 3CO 2 . 5.67 g Fe 2 O 3 x 1 mole x 4 mole Fe x 55.8 g = 3.96 g Fe

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• ### HomeMacarthur Minerals

Macarthur is an iron ore development gold and lithium exploration company that is focused on bringing to production its Western Australia iron ore projects. The Lake Giles Iron Project mineral resources include the Ularring hematite resource (approved for development) comprising Indicated resources of 54.5 million tonnes at 47.2 Fe and

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• ### calculation Questions deducing molecular formula from

AND don t forget to be able to think calculate and deduce the other way round e.g. (i) Suppose a hydrocarbon molecule has an empirical formula of C 2 H 5 and a molecular mass of 58 (C = 12 H = 1). Deduce its molecular formula. The empirical formula mass = (2 x 12) 5 = 29. Dividing 58 by 29 gives 2.

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• ### Can some1 show me how to workout this problem Yahoo Answers

Jan 29 2011 · One of the reactions that occurs in a blast furnace where iron ore is converted to cast iron is Fe2O3 3CO 2Fe 3CO2 Suppose that 1.64 x 103 kg of Fe are obtained from a 2.62 x 103 kg sample of Fe2O3. Assuming that the reaction goes to completion what is the percent purity of Fe2O3 in the original sample My answer is 4.9 x 1o -4 .

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• ### Extracting ironIron and aluminiumGCSE Chemistry

in a huge container called a blast furnace. Iron ores such as haematite contain iron(III) oxide Fe 2 O 3.The oxygen must be removed from the iron(III) oxide in order to leave the iron behind.

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• ### Worksheet #1 Stoichiometry

Calculate the theoretical yield in grams of Fe produced by the reaction of 5.67 g of iron III oxide. If the actual yield is 2.00 g calculate the percentage yield. 2Fe 2 O 3 3C → 4Fe 3CO 2 . 5.67 g Fe 2 O 3 x 1 mole x 4 mole Fe x 55.8 g = 3.96 g Fe

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