Wednesday
April 16, 2014

Search: Given: *Fe2O3(s)+3CO(s)

Number of results: 26,432

chemistry
Fe2O3(s)+3CO(g)--->2Fe(s)+3CO2(g) we see that this chemical equation is already balanced. to get the number of moles of CO, we multiply the given moles of Fe2O3 by the stoichiometric ration from the balanced equation,, thu 1.75 mol Fe2O3 * ( 3 mol CO / 1 mol Fe2O3 ) = 5.25 ...
Monday, April 11, 2011 at 7:34am by Jai

chemistry 2
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 iron in grams that can bbe obtained from 454g (1.00 lb) of iron (III) oxide? AND what mass of CO is required to react with the 454g of Fe2O3? ...
Sunday, October 9, 2011 at 12:14pm by cheryl

CHEMISTRY
Fe2O3 + 3CO= 2Fe + 3CO2, SUPPOSE THAT 1.64kg OF Fe ARE OBTAINED FROM A 2.62kg SAMPLE OF Fe2O3(ORE). ASSUMING THE REACTION IS COMPLETE, WHAT IS THE PERCENT PURITY OF THE Fe2O3 IN THE ORIGINAL SAMPLE?
Sunday, April 17, 2011 at 11:50am by BECKY

chemistry
Fe2O3+ 3CO=2Fe+3Co2, suppose that 1.64kg of Fe are obtained from a 2.62kg sample of Fe2O3 (ore). assuming that the reaction goes to completion, what is the percent purity of the Fe2O3 in the original sample.
Tuesday, April 19, 2011 at 12:26pm by becky

Chenmistry
Fe2O3 + 3C = 2Fe + 3CO How many grams of C are required to react with 2.50 moles of Fe2O3 ?
Monday, April 1, 2013 at 9:05pm by Marcie

Chemistry
How many grams of CO are needed to react with an excess of Fe2O3 to produce 233.4 gFe? Fe2O3 (s) + 3CO (g) --> 3CO2 (g) + 2Fe (s)
Sunday, December 11, 2011 at 8:37pm by :)

chemistry
how many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7gFe? Fe2O3(s) + 3CO(g) => 3CO2(g) + 2Fe(s)
Thursday, January 31, 2008 at 9:41pm by Theodore

chemistry
how many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7gFe? Fe2O3(s) + 3CO(g) => 3CO2(g) + 2Fe(s)
Thursday, March 29, 2012 at 6:25am by help please

Chemistry
How many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7gFe? Fe2O3(s) + 3CO(g) => 3CO2(g) + 2Fe(s)
Thursday, May 17, 2012 at 11:58am by Shelly

chemistry
how many grams of CO are needed to react with an excess of Fe2O3 to produce 201.1 g Fe? Fe2o3(s) + 3CO(g) -> 3CO2(g) + 2Fe(s)
Sunday, April 28, 2013 at 9:46pm by daniele

Chemistry
Use the balanced equation to determine the theoretical yield. Focus on the chemicals whose quantities you are given or are asked to find. CO is not important as it is excess and will make sure that all of the Fe2O3 will be changed to iron. Remember the quotients (numbers in ...
Sunday, March 28, 2010 at 6:16pm by Hanna

chemistry
The coefficients tell you. First, balance it. Fe2O3 + 3CO ==>2Fe + 3CO2 1 mol Fe2O3 = 3 moles CO = 2 moles Fe = 3 moles CO2
Tuesday, September 20, 2011 at 1:48pm by DrBob222

chemistry
Fe2O3 + 3CO --> 2Fe + 3CO2 a 16.2 L sample of CO at 1.5 atm and 200 C is combind with 15.39 g Fe2O3. how many moles of CO are available for the reaction? what is the limiting reacta? How many moles of Fe are formed?
Wednesday, March 10, 2010 at 5:29pm by hilde

Chemistry
How much heat (in kilojoules) is evolved or absorbed in the reaction of 2.90g of Fe2O3 with enough carbon monoxide to produce iron metal? Fe2O3 + 3CO ---> 2Fe + 3CO2 dH=-24.8kJ How do you find q (of the 2Fe in kJ).
Wednesday, April 6, 2011 at 6:00pm by Chris

Chemistry
Can you balance this equation please? Fe2O3 + CO yeilds Fe + CO2 Fe2O3 + CO ==> Fe + CO2 Rule: balance by changing coefficients. You may not change subscripts. Look at the Fe atoms. There are 2 Fe atoms on the left and only 1 on the right; therefore, we place a 2 in front ...
Tuesday, February 20, 2007 at 5:38pm by mZ. YoU

Chemistry
Fe2O3 + 3CO ==>2Fe + 3CO2
Saturday, November 19, 2011 at 9:05pm by DrBob222

Chemistry
Fe2O3(l) + 3CO(g) heat ==>2Fe(l) + 3CO2(g) mols Fe2O3 = grams/molar mass Convert mols Fe2O3 to mols Fe using the coefficients in the balanced equation. Convert mols Fe to g. g = mols x molar mass You will obtain the same answer as my short answer above.
Monday, March 18, 2013 at 3:21pm by DrBob222

Chem
Calculate the number of grams of Fe formed when 0.300kg of Fe2O3 reacts. Equation: Fe2O3+CO-->Fe+CO2 converted .300kg to 300g Balanced Fe2O3+3CO-->2Fe+3CO2 So I started by trying this: 300gFe2O3(1molFe2O3/159.687gFe2O3)...and then I don't know where I would go from there...
Sunday, September 16, 2012 at 10:04pm by Ezra

Chemistry
Which element is oxidized in this reaction? Fe2O3+ 3CO-(arrow)2Fe+3CO2
Monday, October 5, 2009 at 1:08am by Rose

stoichiometry
1.how many mole, Fe can be made from Fe2O3 by the use of 20 moles of carbon monoxide, CO in the following reaction? Fe2O3+ 3CO = 2Fe+ 3CO2 2. How manhy moles of H2O are produced when 2.75 moles of O2 are consumed if burning methyl alcohol, CH3OH, according to the following ...
Saturday, April 6, 2013 at 2:34pm by jace

college
In the reaction Fe2O3 + 3CO 2Fe + 3CO2 How much CO is used to produce 112 grams of iron?
Monday, July 12, 2010 at 12:44pm by Dillon

chemistry
In the reaction Fe2O3 + 3CO 2Fe + 3CO2 How much CO is used to produce 112 grams of iron?
Tuesday, July 13, 2010 at 6:58am by Dillon

Chemistry
Iron metal is formed during the reduction of iron(III) oxide: Fe2O3 + 3CO 2Fe + 3CO2 When 24.3 kg of Fe2O3 react with 14.6 kg of CO and 7.8 kg of Fe are recovered, what is the percent yield for the reaction? Pls.. help I am having a hard time finding the answer. The wordings ...
Wednesday, April 13, 2011 at 11:45pm by komal

Thermochemistry
3CO(g)+ Fe2O3(s) --> 2Fe(s) + 3CO2(g) + 24.7 kJ. How much heat is released when 56 grams of CO react?
Tuesday, December 14, 2010 at 11:22pm by Hannah

Chemistry
Given the balanced equation: a. Fe2O3+3C=2Fe+3CO: b. How many moles of Fe are produced when 1.36 moles of carbon monoxide are produced? c. How many grams of Fe is part b equal to? d. how many molecules of Fe are in part B
Monday, October 8, 2012 at 4:50pm by Noel

Chemistry
Iron(III) oxide can be reduced by carbon monoxide. Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. Substance: Fe2O3(s) CO(g) Fe(s) CO2(g) ΔH f (kJ/mol): -824.2 -110.5 0 -393.5 &#...
Thursday, March 31, 2011 at 5:56pm by Bea

AP Chemistry
Given: m{sample} = 40.3g m{Fe2O3} = 10.5g w{Fe2O3} = 159.6887 0.0002 g/mol w{Fe} = 55.8452 0.0001 g/mol And the stoichiometry: m{Fe}/w{Fe} = 3 m{Fe2O3}/w{Fe2O3} The percentage of iron in the sample is: m{Fe}/m{sample} = ...
Friday, August 30, 2013 at 9:52pm by Graham

chemistry
Fe2O3 + 3CO --> 2Fe + 3CO2. I remind you that in iron(III) oxide, the III are capital "eyes" and not "ones".
Saturday, October 30, 2010 at 1:22pm by DrBob222

Chemistry
Fe2O3 + 3CO --> 2Fe + 3CO2 This one is difficult, took me about 10 minutes, but it's pretty simple in a way that you just plug in number and do trial and errors...
Sunday, January 6, 2008 at 5:36pm by Jake1214

AP Chemistry
Given: m{sample} = 40.93g m{Fe2O3} = 30.7g w{Fe2O3} = 159.6887 0.0002 g/mol w{Fe3O4} = 231.5333 0.0003 g/mol And the stoichiometry: 3 m{Fe3O4}/w{Fe3O4} = 2 m{Fe2O3}/w{Fe2O3} The percentage of magnetite in the sample is: m{Fe3O4} / m{sample} = (2/3) m{Fe2O3} w{Fe3O4} / (w{...
Friday, August 30, 2013 at 9:32pm by Graham

chemistry
How many moles of carbon monoxide are needed to react completely with 1.75 moles of iron oxide? based on this equation: Fe2O3(s)+3CO(g)--->2Fe(s)+3CO2(g)
Monday, April 11, 2011 at 7:34am by Jane

Balancing Equations
FeO3 + 3CO = Fe + 3CO
Monday, December 14, 2009 at 5:50pm by Anomynous

chemistry
how much energy is required to convert 1.00 kg of iron III to atomic iron? Equation: Fe2O3 + 3CO ---> 2 Fe +3 CO2 delta H is 131kJ
Wednesday, February 8, 2012 at 8:02pm by David

chemistry
Given: *Fe2O3(s)+3CO(s)-->2Fe(s)+3CO2(g)(delta h is -23kJ) *3Fe2O3(s)+CO(g)-->2Fe3O4(s)+CO2(g)(delta h is -39kJ) *Fe3O4(s)+CO(g)-->3FeO(s)+CO2 (delta h is 18kJ) Desired:FeO(s)+CO(g)-->Fe(s)+CO2(g) find delta h for the desired reaction. which reactions do i reverse ...
Wednesday, March 26, 2008 at 10:08pm by tanisha

Chemistry
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?
Sunday, March 28, 2010 at 6:16pm by Kim

Chemistry
how many moles Fe in 112g? each 2 moles of Fe uses 3 moles CO Generally, "^" are not used in molecular formulas. Better would be Fe2O3+3CO->2Fe+3CO2
Wednesday, March 6, 2013 at 5:09pm by Steve

AP Chemistry
Amount of Iron in sample: n[Fe] = 3 m[Fe3O4]/w[Fe3O4] Amount of Iron in assay: n[Fe] = 2 m[Fe2O3]/w[Fe2O3] The amount of iron is conserved, so: m[Fe3O4] = (2/3) m[Fe2O3] w[Fe3O4] / w[Fe2O3] Substitute: m[Fe2O3] = 26g w[Fe2O3] = 159.6887 0.0002 g/mol w[Fe3O4] = 231.5333 0....
Friday, August 30, 2013 at 7:31pm by Graham

Chemistry
In the reaction Fe^2O^3+3CO->2FE+3CO^2, what is the total number of moles of CO used to produce 112 grams of iron? Please explain step by step how to do this problem, thanks:)
Wednesday, March 6, 2013 at 5:09pm by Unknownn

Chimestry
533 kg Fe x (Fe2O3/2*Fe) = 533 kg x (159.69/2*55.85) = ? kg Fe2O3 and substitute this into the below. %Fe2O3 = (?mass Fe2O3/950kg)*100 = ? %
Tuesday, September 11, 2012 at 4:33pm by DrBob222

Chemistry
Label the oxidizing agent and the reducing agent: a) P4(s) + 5O2(g) -> P4O10(s) b) Co(s) + Cl2(g) -> CoCl2(s) c) Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g) d) PbS(s) + 4H2O2(aq) -> PbSO4(s) + 4H2O(l) I never learned about oxidation numbers. Thanks!
Wednesday, September 3, 2008 at 12:32am by Yuval

chemistry
21.3 g Fe2O3 x (1 mol Fe2O3/molar mass Fe2O3) x (2 mol Fe/1 mol Fe2O3) x (atomic mass Fe/1 mol Fe) = g Fe Note: There is an easier way to do this if you use the chemical factor; however, schools don't teach that anymore. 21.3 x *(2Fe/Fe2O3) = 21.3 x (2*55.85/159.6) = ? g Fe.
Sunday, September 2, 2012 at 6:09pm by DrBob222

AP Chemistry
Find the number of moles of Fe2O3 in 10.5g of Fe2O3: 10.5g*(1 mole/159.6882 g)=moles of Fe2O3 Convert moles of Fe2O3 into moles of Fe: Moles of Fe2O3*(2 moles of Fe/1 mole of Fe2O3)=moles of Fe How many g of Fe are in the moles of Fe calculated above? Moles of Fe*(55.845g/...
Friday, August 30, 2013 at 9:52pm by Devron

Chimestry
Because thee are two Fe atoms in one molecule of Fe2O3. 533 kg Fe x (1 mol Fe/55.85 g Fe) x (1 mol Fe2O3/2 mols Fe) x (159.69 g Fe2O3/1 mol Fe2O3) = ?kg Fe2O3. Note all of the units cancel and you are left with 533 x [159.69/(2*55.85)] = ? kg Fe2O3.
Tuesday, September 11, 2012 at 4:33pm by DrBob222

chemistry
I would use the dimensional analysis approach. Start with what you have (in this case 15 mols Fe2O3) and convert to mols CO2. 15 mols Fe2O3 x (3 mols CO2/2 mols Fe2O3) = ?? Notice that the 3 mols CO2 and 2 mols Fe2O3 come form your equation. Also notice that mole Fe2O3 you ...
Wednesday, April 9, 2008 at 2:09pm by DrBob222

Chemistry
213.5g Fe2O3 x (1 mole Fe2O3/molar mass Fe2O3) x (3 atoms oxygen/1 mole Fe2O3) x (16 g oxygen/1 mole O atoms) =
Monday, January 17, 2011 at 7:23pm by DrBob222

AP Chemistry
Not sure how to be clearer. From the formula, the mole amount of iron in the magnetite sample is three times the mole amount of iron(II,III) oxide. This amount is the mass of magnetite divided by its molar weight. n[Fe] = 3 m[Fe3O4]/w[Fe3O4] The amount of iron in the converted...
Friday, August 30, 2013 at 7:31pm by Graham

Chemistry
1.) What are the equilibrium partial pressures of CO and CO2 if co is the gas present initially, at a partial pressure of .912 atm. Kp = 19.9 Fe2O3 + 3CO <--> 2Fe + 3CO2 I'm trying to find partial pressure of both CO and CO2 by calculating for "x" in the equilibrium problem
Tuesday, May 8, 2012 at 12:51pm by Ali

chemistry check
please check Write the balanced equation, with the enthalpy component, for the rusting process, given that Hf for iron and oxygen is 0 and Hf for ferric oxide is -826 kJ/mol. 4 Fe (s) + 3 O2 (g) --------> 2 Fe2O3 (s) You need to add the heat one of three ways. 4 Fe (s) + 3 ...
Thursday, February 8, 2007 at 9:35am by key

chemistry
First, you must balance the equation. (I assume you must balance the equation; it doesn't make sense to list mol ratios for equations that won't work.) Then you look at the coefficients of the material in the equation. Fe2O3 + 3CO ==> 2Fe + 3CO2 Now, carbon monoxide, CO, is...
Friday, February 29, 2008 at 4:11pm by DrBob222

chemistry
Back track, 45.8 grams of Fe2O3*(1 mole/159.69 g)= moles of Fe2O3 moles of Fe2O3 *(3 moles of O2/2 moles of Fe2O3)=moles of O2 moles of O2*(32.0g of O2/1mole)= mass of O2
Wednesday, February 27, 2013 at 12:03pm by Devron

Honors Chemistry
Equation: Fe2O3 + 2Al ---> 2Fe + Al2O3. How many grams of Fe2O3 react with excess Al to make 475g Fe? Can you show me step by step how to do it? My book says the answer is 679g Fe2O3.
Tuesday, February 23, 2010 at 9:38pm by Anan

chemistry
2Al + Fe2O3 ==> 2Fe + Al2O3 You must know the delta H of the reaction. Make sure it is kJ/rxn and not kJ/mol. It takes 27 x 2 = 54 g Al to produce the kJ for delta Hrxn. 54 g Al x (360 kJ/deltaHrxn) = g Al required. g Fe2O3 required = g Al x (1 mol Fe2O3/2 mol Al) = g Al x...
Tuesday, April 13, 2010 at 2:15pm by DrBob222

11th grade
so I have this problem and I dont know what numbers to multiple and whatnot. Can someone help me? This is the problem: 4000 g Fe2O3* 1mole Fe2O3/159.68 gFe2O3* 3mole CO2/1mole Fe2O3
Thursday, December 2, 2010 at 4:18pm by Jessi

chem
The molecular formula for iron(III) oxide is Fe2O3. This means that 2 moles of Fe=1 mole of Fe2O3. 22.65g of Fe*( 1 mole of Fe/55.8 g)= moles of Fe moles of Fe*(1 mole of Fe2O3/2 moles of Fe)*(159.69 Fe2O3 g/mol)= mass of the sample
Friday, February 22, 2013 at 2:35pm by Devron

Chemistry!!
The way you have it written the oxygens do not balance. It is actually: 4Fe + 3O2 > 2Fe2O3. (or, 2Fe + 1.5O2 > Fe2O3. So, basically 2 moles of Fe goes to form one mole of Fe2O3. Then, you must calculate how many moles of Fe you start with, and then you know how many ...
Saturday, November 22, 2008 at 12:29pm by DanH

AP chemistry
2Fe(ore) + ???? ==> Fe2O3 + other stuff. mass Fe2O3 = 19.5. Convert to moles Fe2O3. 19.5/160 = 0.122 moles. moles Fe is 0.122 x 2 (there are two moles Fe for every 1 mole Fe2O3) = 0.244 moles Fe. g Fe = moles x molar mass. I estimated the molar mass of Fe2O3. You should ...
Tuesday, August 3, 2010 at 1:40pm by DrBob222

Chemistry
I will save some time by estimating molar masses and using a minimum of numbers. You need to go back through it and redo them exactly. Check all my arithmetic procedures, too. Step 1. Write and balance the equation. Fe2O3 + 3CO ==> 2Fe + 3CO2 Step 2. Convert what you have ...
Friday, February 29, 2008 at 4:10pm by DrBob222

chemistry
iron 3 oxide reacts with carbon monoxide according to the following equation: fe2O3+3Co-->2Fe+3Co2 a) how many moles of ions are produced when one mole of iron 3 oxide reacts b) calculate the volume of carbondioxide produced when one mole of iron 3 oxidereacts
Monday, September 6, 2010 at 4:01pm by honeybee

chemistry
The factor (2*molar mass Fe3O4/3*molar mass Fe2O3) is called the chemical factor. It isn't taught in schools anymore (a mistake I think) because it can be arrived at through another procedure. The entire process is this. 4Fe3O4 + 2O2 ==> 6Fe2O3 + O2 12.5g Fe2O3 x (4 mols ...
Thursday, September 5, 2013 at 7:50pm by DrBob222

Chemistry
Notice the mol cancels out and you're left with grams. (0.250 mol Fe2O3)*(molar mass (in grams) Fe2O3/1 mol Fe2O3)
Friday, April 8, 2011 at 12:29pm by TutorCat

chemistry
Fe2O3(s) + 2CO(g)-->2Fe(s)+ 2CO2(g) Convert 4.00 kg Fe2O3 to moles. moles = grams/molar mass. Now look at the balanced equation. 1 mole Fe2O3 requires 2 moles CO and produces 2 moles Fe and 2 moles CO2.
Thursday, November 5, 2009 at 2:13pm by DrBob222

So very confused :(
Okay so after some trial and error (I just kept trying different things Until I got the answer), I figured out it's *probably* solved like this: Enthalpy = 23.6g Fe2O3 x 1 mol Fe2O3/[(2x56) + (3x16)]g x -1.65x10^3 kJ/2 mol Fe2O3 = -1.22 x 10^2 kJ If that's right, my question ...
Wednesday, February 6, 2013 at 4:39pm by A Canadian

Chemistry
I want to know the enthalpy change for this reaction which occurs in a blast furnace: Fe2O3(s) + 3C(s) --> 2Fe(l) + 3CO(g) You will need the heat of formation for CO, and ironIIIoxide, and the heatofmelting for iron. I suspect you have some temperature in mind also which ...
Sunday, April 15, 2007 at 9:26am by Alice

Chemistry
A 500g iron (Fe) rod was left in air for a long period of time, and got covered with rust (Fe2O3) as a result of reaction with atmospheric oxygen. The mass of the rusty rod was determined as 560g. a) calculate the theoretical yield of Fe2O3(s), that is the mass of Fe2O3(s) ...
Sunday, March 18, 2012 at 8:47pm by Riley

chemistry
You haven't done anything yet except retype the problem. How many moles is in 2.83 g Fe2O3? If 6 moles Fe2O3 uses 392 kJ heat, how much heat would be used by 3 moles Fe2O3? Suppose that would be half of 392? Use the same reasoning to determine heat used by moles in 2.83 g Fe2O3.
Thursday, October 15, 2009 at 11:41pm by DrBob222

Chemistry
4Fe + 3O2 -> 2Fe2O3 + 1.65E3 kJ C) what is the enthalpy change for the formation of 23.6 g of iron(iii) oxide? I'm trying to understand thermochemical reactions and stoichiometry, so could you please tell me if this is correct? And please explain the parts that I clearly ...
Wednesday, February 6, 2013 at 6:45pm by A Canadian

Chemistry
4Fe + 3O2 -> 2Fe2O3 + 1.65E3 kJ C) what is the enthalpy change for the formation of 23.6 g of iron(iii) oxide? I'm trying to understand thermochemical reactions and stoichiometry, so could you please tell me if this is correct? And please explain the parts that I clearly...
Wednesday, February 6, 2013 at 8:46pm by A Canadian

Chemistry
I'm having a hard time figuring these out. Please help me on them! For the reaction Fe2O3 + 3 Co = 2 Fe + 3 CO2: a) how many moles of Fe can be produced from 75 moles Co? b) how many moles of CO2 can be produced from 15 moles of Fe2O3? c) what is the maximum amount (in grams) ...
Wednesday, April 9, 2008 at 4:01pm by Kate

Chemistry
4 FeS(s) + 7 O2(g) ==> 2 Fe2O3(s) + 4 SO2(g) 7.82 moles of FeS are required to produce 3.91 moles of Fe2O3 What is the maximum number of liters of Fe2O3(s) that can be made from 10.95 L of O2(g) and 18.64 L of FeS(s) at STP?
Friday, July 22, 2011 at 4:01pm by Katie

AP Chemistry
Didn't I do this for you (or one similar to it) a couple of days ago. 12.9g x (1 mol Fe2O3/molar mass Fe2O3) x (2 mols Fe/1 mol Fe2O3) x (atomic mass Fe/1 mol Fe) = ? There is an easier way to do this but chemical factors are not taught in most schools now. 12.9 x (2*Fe/Fe2O3...
Monday, September 3, 2012 at 9:56pm by DrBob222

Analytical chemistry
I did the next problem, i don't have the results for it and i just want to know if i calculated the mass for Fe2O3 the right? A sample is a mixture of iron oxides (Fe2O3 and FeOOH). It's known that at 200C this reaction occurs: 2FeOOH(s)-> Fe2O3(s) + H2O(g) A 0.2564g ...
Saturday, September 7, 2013 at 1:54pm by Gloria

Chem
This is a limiting reagent. You know that because BOTH of the reactant are given. First, balance the equation. Convert 147 g FeS2 to moles. moles = grams/molar mass. Convert 88 g oxygen to moles. Using the coefficients in the balanced equation, convert moles FeS2 to moles ...
Sunday, September 19, 2010 at 9:19pm by DrBob222

chemistry (grade 12)
This is a combination limiting reagent problem with heat thrown in for good measure. What is the limiting reagent? How much Fe2O3 reacts? 851.5 kJ x (g Fe2O3 reacting/molar mass Fe2O3) = kJ heat released.
Wednesday, February 15, 2012 at 3:20pm by DrBob222

Chemistry
There are 6.022E23 molecules of Fe2O3 in 159.69 g (1 mole) Fe2O3.
Wednesday, June 15, 2011 at 3:23pm by DrBob222

Chemistry
the density of Fe2O3 is 5.343g cc. What is the mass volume concentration of iron in Fe2O3
Wednesday, October 16, 2013 at 9:19pm by jay

Chemistry
How many grams of Fe2O3 are there in 0.250 mole of Fe2O3?
Friday, April 8, 2011 at 12:29pm by Anonymous

chemistry
how grams of oxygen can be produced from the decomposition of 100g KClO3? how much iron can be recovered from 25.0g of Fe2O3 how can be produced from 125g Ag2S Figure the precentage composition of the compound. For instance percent of Fe in Fe2O3 = 2*atomicmassFe/(...
Monday, February 26, 2007 at 5:31pm by Beautiful

Chemistry
A sample weighing 3.064 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not react. If the sample residue weighs 2.407 g, ...
Monday, October 29, 2012 at 2:23am by Chris

Chemistry
Actually, the mass of Fe in the residue is 2.407-Al2O3. The Fe2O3 has all lost its oxygen, leaving only Fe. So, if you started out with x moles of Fe2O3 and y grams of Al2O3, then converting the Fe2O3 to grams, 159.69x + y = 3.064 55.85(2x) + y = 2.407 The equations may look a...
Monday, October 29, 2012 at 2:23am by Steve

AP Chem
The simple way is to convert mass Fe2O3 into mass Fe3O4 by using a chemical factor (which is not taught anymore). mass Fe2O3 x (2*molar mass Fe3O4/3*molar mass Fe2O3) = ??
Wednesday, August 24, 2011 at 9:08pm by DrBob222

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. Calculate the percent Fe2O3 in the sample. the mass i get for fe2o3 is too big, but i don't know how else to do this problem, someone please help :S ...
Saturday, August 3, 2013 at 1:40pm by Gloria

Chemistry
A sample of iron weighing 15.0 g was heated with potassium chlorate (KClO3) in an evacuated container. The oxygen generated from the decomposition of KClO3 converted some of the Fe to Fe2O3. If the combined mass of Fe and Fe2O3 was 17.9g,calculate the mass of Fe2O3 formed and ...
Thursday, August 22, 2013 at 10:30pm by Francis

Chemeistry
(4.50g Fe2O3)*(1mol Fe2O3/159.7g Fe2O3)*(111.69g Fe2/1mol Fe2)= 3.15g Fe2 %Yield = (2.60g/3.15g)*100 = 0.825*100 = 82.5%
Monday, March 25, 2013 at 10:46pm by Goon

chemistry
Your answer leaves me with 1.63 so is this wrong moles oxalic acid = 0.500 L x 0.122 M=0.610 the ratio between Fe2O3 and H2C2O4 is 1 : 6 moles Fe2O3 = 0.610/6=0.102 mass Fe2O3 = 0.102 mol x 159.69 g/mol=16.3 g It left me with 16.3
Monday, October 4, 2010 at 8:49am by amber

Chemistry ( stoichiometry )
How many grams of iron can be made from 16.5g of Fe2O3 by the following equation: Fe2O3 + 3 H2 -----> 2 Fe + 3 H2O.
Wednesday, November 10, 2010 at 8:33pm by Sevi

Chemistry-Stoichiometry
0.1 mol Fe x (2 mol Fe2O3/4 mol Fe) = 0.1 x 1/2 = 0.05 mol Fe2O3 produced if we had 0.1 mol Fe and all the O2 we needed. 0.16 mol O2 x (2 mol Fe2O3/3 mol O2) = 0.16 x 2/3 = 0.107 mol Fe2O3 produced if we had 0.16 mol O2 and all the Fe we needed. So Fe must be the limiting ...
Saturday, October 19, 2013 at 3:41am by DrBob222

Chemistry
It's 1.65 x 10^3 kJ. This is what I did for the 1st question: -0.250 kg Fe x 1g Fe/10^3 kg x 1 mol Fe/223.4 g Fe x -1.65 x 10^3 kJ/4 mol Fe = 4.61 x 10^-4 kJ Fe 2nd question: 2.00 x 10^3 kJ Fe2O3 x 2 mol Fe2O3/ -1.65 x 10^3 kJ x 319.4 g Fe2O3/1 mol Fe2O3 = -774.3 g Fe2O3
Sunday, February 21, 2010 at 11:31pm by Kaylene

Chemeistry
when 4.50 g of fe2o3 is reduced with excess h2 in a furnace, 2.6 g of iron metal is recovered. What is the percent yield when molar mass of Fe2O3 is 159.7
Monday, March 25, 2013 at 10:46pm by Sammy

Chemistry
Fe2O3(s) + 2Al(s)-> 2Fe(l) + Al2O3(s) What is the theoretical yield of iron if we begin the reaction with 10.5 g of Al (assume an excess of Fe2O3)
Sunday, February 16, 2014 at 8:18pm by tgt

Chemistry
Your original equation is not balanced. It should be 2 Fe2O3 + 3 Co = 2 Fe + 3 CO2 a) The Fe:Co mole ratio is 2:3 Use that fact to do the calculation b) The CO2:Fe2O3 mole ratio is 3:2 c) Convert 454 g of Fe2O3 to moles. You will produce 1.5 times as many moles of CO2. Convert...
Wednesday, April 9, 2008 at 4:01pm by drwls

chemistry
mols Cr2O7^2- = M x L = ? Convert moles Cr2O7^2- to mol Fe. mols Fe = mols Cr2O7^2- x (6 mol Fe/1 mol Cr2O7^2-) = ? (from the equation) Convert to moles Fe2O3. mol Fe x (1 mol Fe2O3/2 moles Fe) = ? g Fe2O3 = moles Fe2O3 x molar mass = ? %Fe2O3 = (mass Fe2O3/mass sample)*100 = ?
Wednesday, February 15, 2012 at 5:17pm by DrBob222

chem
One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron, is below. Fe2O3 + 3 CO 2 Fe + 3 CO2 Suppose that 1.86 103 kg of Fe are obtained from a 5.98 103 kg sample of Fe2O3. Assuming that the reaction goes to completion, what is the percent...
Tuesday, August 7, 2012 at 3:25pm by Shawn

Chemistry-Equations
1. Write and balance the equation. 4Fe + 3O2 ==> 2Fe2O3 2. Convert what you have (in this case 16.7 g Fe) to moles. moles = grams/molar mass. 3. Using the coefficients in the balanced equation, convert moles of what you have (Fe) to moles of what you want (in this case ...
Friday, March 5, 2010 at 11:27am by DrBob222

chemistry
200 g x 0.50 = ?? g Fe2O3. moles Fe2O3 = ??g/molar mass Fe2O3. moles Fe = 3 x moles Fe2O3. g Fe = moles Fe x molar mass Fe.
Thursday, October 7, 2010 at 10:48pm by DrBob222

Chemistry
For Fe2O3. (2*atomic mass Fe/molar mass Fe2O3)*100 = ? The others are done the same way.
Wednesday, March 5, 2014 at 11:59am by DrBob222

chemistry
6Na+Fe2O3=3Na2O+2Fe if Interact 100g of Na with 100g of Fe2O3,Calculate: - The resulting mass of iron?
Tuesday, February 4, 2014 at 10:05am by Anonymous

chemistry (grade 12)
how much heat will be liberated if 37.8 g of Fe2O3 is allowed to react with 18.7 g of aluminum. Fe2O3(s) + 2Al(s)--> Al2O3(s) + 2Fe(s) + 851.5kJ
Wednesday, February 15, 2012 at 3:20pm by Rose Bud

Chemistry
This isn't exactly a homework question, I'm just trying to understand the concept we learned today... So say we had: 4Fe + 3O2 → 2Fe2O3 + 1.65 x 10^3 kJ Does that mean for every 4 mol of Fe, 3 mol of O2, and 2 mol of Fe2O3 we have 1.65 x 10^3 kJ? And if I were to ...
Wednesday, February 6, 2013 at 4:39pm by A Canadian

science
How many grams of CO are needed to react with an excess of Fe2O3 to produce 558 g Fe? The equation for the reaction is: Fe2O3(s) + 2 CO(g) → 3 CO2(g) + 2 Fe(s)
Tuesday, January 11, 2011 at 2:11am by christopher

Chemistry
%Fe = (g Fe in sample/mass sample)*100. You know mass sample. Calculate g Fe. 0.1116 g Fe2O3 x (2 moles Fe/1 mole Fe2O3) = 0.1116 x (2*55.85/molar mass Fe2O3) = xx g Fe. Substitute into the first equation and obtain %Fe.
Tuesday, September 14, 2010 at 8:07pm by DrBob222

Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>

Search
Members