An alternative method for preparing pure iron from Fe2O3 is by reaction with carbon monoxide: ...
Question:
An alternative method for preparing pure iron from {eq}Fe_2O_3{/eq} is by reaction with carbon monoxide:
{eq}Fe_2O_3 + CO \rightarrow Fe + CO_2 {/eq}
How many grams of CO are needed to react with 3.12 g of {eq}Fe_2O_3{/eq}?
Express the answer using three significant figures.
Carbon Monoxide & Carbon Dioxide:
Both carbon monoxide and carbon dioxide are oxides of carbon. In carbon monoxide, the oxidation state of carbon is +2. In carbon dioxide, the oxidation state of carbon dioxide is +4. Carbon is incompletely oxidized to produce carbon monoxide. However, the complete oxidation of carbon leads to the formation of carbon dioxide.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe balanced chemical equation is shown below:
{eq}\rm Fe_2O_3+3CO\to 2Fe+3CO_2 {/eq}
The molar mass of {eq}\rm Fe_2O_3 {/eq} is 159.69 g/mol....
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Mole-to-Mole Ratios and Calculations of a Chemical Equation
from
Chapter 9 / Lesson 2
155K
Learn about the mole ratio. Understand the definition of mole ratio, how to find mole ratio in stoichiometry, and see examples of using mole ratio in problems.
Related to this Question
- Iron (III) oxide reacts with carbon to given iron and carbon monoxide: Fe_2O_3 (s) + 3C(s) to 2Fe(s) + 3CO(g). How many grams of C are required to react with 10.4 g of Fe_2O_3?
- Iron (III) oxide reacts with carbon to give iron and carbon monoxide: F{e_2}{O_3}\left( s \right) + 3C\left( s \right) \to 2Fe\left( s \right) + 3CO\left( g \right) a. How many grams of C are required to react with 10.4 g of F{e_2}{O_3}?
- Iron(III) oxide reacts with carbon to give iron and carbon monoxide: Fe2O3(s) + 3C(s) -> 2Fe(s) + 3CO(g) How many grams of C are required to react with 10.4 g of Fe2O3?
- 448g of iron(III) oxide, Fe2O3, reacts with an excess of carbon monoxide, CO in the following reaction. Fe2O3(s)+3CO(g) yields 2Fe(s)+3CO2(g) a) Calculate the mass of iron solid, Fe, produced and use the following molar masses in your calculation: Fe2O3=
- Iron three oxide reacts with carbon to give iron and carbon monoxide. How many grams of Fe can be produced when 6.50 g of Fe_2O_3 reacts?
- Combining 0.235 mol Fe2O3 with excess C produced 18.5 g Fe based on the following reaction: Fe2O3 + 3C to 2Fe + 3CO. What is the actual yield of Fe in mol?
- How many grams of FE2O3 are there in 0.500 mole of FE2O3?
- You are working on ways to improve the process of changing iron ore (Fe_2O_3) into pure iron. Fe_2O_3 + 3CO rightarrow 2Fe + 3CO_2 a. If you start with 150 g of Fe_2O_3 as limiting reactant, how many molecules of Fe_2O_3 do you start with? b. How many mol
- Balance the equation below and answer the question. Fe + O2 arrow Fe2O3 How many grams of Fe2O3 are produced when 2.93 x 1011 molecules of O2 are reacted?
- 448g of iron(III) oxide, Fe2O3, reacts with an excess of carbon monoxide, CO in the following reaction. Fe2O3(s)+3CO(g) yields 2Fe(s)+3CO2(g). Find the percentage yield if only 243.5g of Fe is actually isolated. Use the following molar masses in your cal
- Combining 0.292 moles of Fe2O3 with excess carbon produced 15.4 grams of Fe. Fe2O3 + 3C arrow 2Fe + 3CO a. What is the actual yield of iron in moles? b. What is the theoretical yield of iron in moles?
- Unbalanced reaction: Fe + O_{2} \rightarrow FE_{2}O_{3}. \Delta H = -1652 kJ a. How much heat is involved when 100. g of iron reacts? b. How much heat is involved when 100. g of Fe_{2}O_{3} is produced? c. How many grams of oxygen did you start with when
- Consider the balanced chemical reaction below. How many grams of carbon monoxide are required to react with 6.4 g of iron (III) oxide? Set up a table below to determine the minimum number of moles of CO required to react with the Fe_2 O_3 and then determ
- The process for reducing iron ore to iron metal is: \begin{matrix} & Fe_2O_{3 (s)} + & 3CO_{(g)} \to & 2Fe_{(s)} + & 3CO_{2 (g)} \\\textrm{MM} & 159.6 & 28 & 55.8 & 44\end{matrix} How many moles of CO are needed to make 0.28 moles of CO_2? Answer to the
- Iron(III) oxide reacts with carbon to give iron and carbon monoxide: Fe2O3(s) + 3C(s) -> 2Fe(s) + 3CO(g) How many grams of CO when 34.0 g of C reacts?
- In the reaction given below, for every two moles of iron(III) oxide consumed, how many moles of iron are produced? 2 Fe2O3 4 Fe + 3 O2
- Calculate the mass of H2O in the following reaction, if 116.3 grams of Fe2O3 and 10.5g of 3H2 are used.
- Combining 0.251 moles of Fe2O3 with excess carbon produced 181 grams of Fe. Fe2O3 + 3C arrow 2Fe + 3CO a. What is the actual yield of iron in moles? b. What is the theoretical yield of iron in moles? c. What is the percent yield?
- Iron(III) oxide reacts with carbon to give iron and carbon monoxide: Fe2O3(s) + 3C(s) -> 2Fe(s) + 3CO(g) How many grams of CO are produced when 34.0 g of C reacts?
- How many grams of O2 are needed to produce 0.400 mole of Fe2O3?
- Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s) + 3CO(g) arrow 2Fe(s) + 3CO2(g) What is the percent yield for iron if the reaction of 70.0 grams of iron(III) oxide produces 38.0 grams of iron?
- Iron is produced in a blast furnace from the reaction of iron (III) oxide with carbon monoxide. The products of the reaction are iron and carbon dioxide. The balanced chemical reaction is shown below. How many kilograms of iron may be formed when 1.63 \ti
- To make pure iron metal from its ore, iron(III) oxide must react with carbon monoxide. The products of this reaction are iron metal and carbon dioxide gas. The balanced chemical equation for this reaction is given below. Fe2O3 + 3CO arrow 2Fe + 3CO2 Suppo
- What mass of iron(III) oxide would be required to produce 2250g of iron metal? How many moles of carbon monoxide would be used during this reaction?
- Determine the limiting reactant when 80.0 grams of Fe2O3 are reacted with 36.0 grams of CO in the following reaction. Fe2O3(s) + 3CO(g) arrow 2Fe(s) + 3CO2(g)
- Calculate the percent of iron in the following compounds: A) FeO B) Fe_2O_3 C) FeCl_3
- What is the percent yield of iron if the reaction of 64.7 g of iron (III) oxide produces 14.2 g of iron? Express your answer to three significant figures.
- How many moles are in 37.8 g of Fe_2O_3?
- Calculate the limiting reactant if 1.50 mol Fe_2O_3 reacts with 2.50 mol Al
- For the following reaction, 20.1 grams of iron are allowed to react with 10.6 grams of oxygen gas. iron(s) + oxygen(g) iron(II) oxide(s) a) What is the maximum mass of iron(II) oxide that can be formed? b) What is the formula for the limiting reagent? c)
- Using the equation 4fe + 3O2 2Fe2O3, if 6 moles of oxygen and an excess of iron were available, how many moles of iron (III) oxide would be produced?
- How many moles of oxygen ions are in 9.47 grams of Fe2O3?
- How many grams of iron are needed to completely consume 2.54 L of oxygen gas according to the following reaction at 25 degrees Celsius and 1 atm? iron (s) + oxygen (g) arrow iron(II) oxide (s)
- If 80 g of Al and 80 g of Fe2O3 are combined, what is the maximum number of moles of Fe can be produced given the reaction 2Al+Fe2O3 --> Al2O3+2Fe?
- What mass of FeCl_3 is required to prepare 100 mL of 0.250 M FeCl_3 solution?
- In a lab, 6.59 g of Iron is combined with Oxygen to produce 6.93 grams of Iron Oxide. Using the two balanced equations for Iron Oxide, 2Fe + O_2 = 2FeO and 4Fe +3O_2 = 2Fe_2O_3, find the theoretical and percent yield for each equation.
- a) Write a balanced equation for the reduction of iron ore (Fe_2O_3) to iron using hydrogen by applying the method of half-reactions. b) What mass of iron would you get from one tonne of ore? c) What is the oxidation state of the iron in Fe_2O_3?
- Write a balanced equation for the reduction of iron ore (Fe_2O_3) to iron, using hydrogen, by applying the method of half-reactions.
- If 1.173 grams of iron in the form of steel wool is placed in a bottle containing 0.021 moles of oxygen, what is the maximum mass in grams of iron(III) oxide that can be produced? 4Fe(s) + 3O2(g) arrow 2Fe2O3(s)
- Consider the reaction 4FeS_2+11O_2 \rightarrow 2Fe_2O_3+8SO_2 a) How many moles of SO_2 can be obtained from 3.0 moles of O_2? b) How many moles of Fe_2O_3 can be obtained from 3.0 moles of O_2?
- An oxide of iron has the formula Fe3O4. What mass percent of iron does it contain?
- A thermite reaction occurs between solid aluminum and iron III oxide (rust) to form molten iron metal and aluminum oxide. 2 Al (s) + Fe2O3 (s) → 2Fe (l) + Al2O3 (s) How many grams of iron are produced for every 1.50 moles of iron III oxide tha
- Iron is in the earth in the form of iron ore. Common ores include Fe_2O_3 (hematite), Fe_3O_4 (magnetite) and FeCO_3 (siderite). Calculate the mass percent composition of iron for each of these iron ores. Which one has the highest iron content?
- Use the following equation: 4Fe(g) + 3O_2 (g) \to 2Fe_2O_3(s) If 32 moles of Fe and 27 moles of O_2 are reacted, which is the limiting reagent?
- In using the thermite reaction, 144 grams of Al are reacted with 155 grams of iron (lll) oxide. How much of excess reagent is left at the end of the reaction?
- FeCl3 reacts with Na5P3O10 to produce Fe5(P3O10)3 according to the following equation: 5FeCl3(aq) + 3Na5P3O10(aq) arrow Fe5(P3O10)3(s) + 15NaCl(aq) (a) Which reactant is limiting if 3.069 grams of FeCl3 and 3.243 grams of Na5P3O10 are allowed to react? (b
- How many moles of Fe3+ are in 500 mL of a 2.00 M FeCl3 solution?
- Balance the following chemical equation and determine the number of moles of Fe(s) produced when 6.9 times 10 -1 moles of Fe_2O_3(s) react with excess C(s) to produce Fe(s) and CO_2(g). Fe_2O_3(s) + C(s) rightarrow Fe(s) + CO_2(g)
- Iron, like most metals, does not occur naturally as the pure metal. Rather, it must be produced from iron ore, which contains iron (III) oxide, according to the given balanced equation. F e 2 O 3 ( s ) + 3 C O ( g ) 2 F e ( s ) + 3 C O 2 ( g ) a. How
- If you have 155 mL of a 0.762 M FeCl3 solution, how many grams of FeCl3 are contained in this sample?
- What mass of iron is required to react completely with 525 ml of 1.6.3 mol/L copper (II) sultans solution?
- If the formula units for Iron(III) oxide is 2.39 \times 10^{24}, then what is the mass of iron (III) oxide? What mass of iron is present in this sample?
- Iron oxide is produced when iron metal is exposed to air, via this process: 3O_2 + 4Fe \rightarrow 2Fe_2O_3 a) Which ion or atom is reduced? b) Which ion or atom is oxidized? c) How many electrons are transferred? d) How many moles of oxygen gas are ne
- If the reaction below causes 0.910 g of silver to be deposited, use atomic masses and the stoichiometric ratio (of coefficients) to determine the moles of silver and iron involved, and the mass of iron involved. (Show all equations with all units and all
- If the reaction below causes 0.910 g of silver to be deposited, use atomic masses and the stoichiometric ratio (of coefficients) to determine the moles of silver and iron involved, and the mass of iron involved. Show all equations with all units and all u
- 10 grams of iron are reacted with 2 grams of oxygen according to the equation below. How much heat will be transferred? Will the heat be absorbed or released? Explain Fully. 4Fe(s) + 3O2 = 2Fe2O3 \\ H = -1652 kJ
- How to find the molar mass of FeCl3
- How many moles of iron are in 4 moles of iron(III) oxide?
- Using the formula : 4Fe(s) +3O_2(g) \rightarrow 2Fe_2O_3(s) If you have 32 moles of Fe and 27 moles of O2, which is the limiting reagent?
- For the reaction shown, calculate how many moles of NO2NO2 form when each amount of reactant completely reacts. 2N2O5(g) 4NO2(g)+O2(g)2N2O5(g) 4NO2(g)+O2(g) a. 5.6 mol of N2O5 - Express your answer using two significant figures. b. 5.13 10^3 mol of N2
- How to balance FeS2 + O2 = Fe2O3 + SO2.
- Consider the following balance equation: 2Fe_2O_3 + 3S \to 3SO_2 + 4Fe. How many moles of sulfur dioxide are made if 12 moles of iron III oxide are used?
- Given the following equation: FeCl2 + 2NaOH rightarrow Fe(OH)2 + 2NaCl, A) If I start the chemical reaction with 3.51 moles of NAOH, how many moles of Fe(OH)2 can I make? B) If I start the chemical reaction with 4.2 moles of FeCl2, how many moles of Fe(OH
- How many grams of iron (iii) chloride will be formed upon the complete reaction of 28.0 grams of chlorine gas with excess iron?
- For the following balanced equation, indicate how many moles and grams of each reactant and product are needed/produced in the reaction if 10.0 grams of FeS2 reacts. 4FeS2 + 11O2 arrow 2Fe2O3 + 8SO2
- Balance this equation: Solid iron(III) oxide and carbon monoxide gas yields iron metal and carbon dioxide gas.
- When iron rusts the iron metal reacts spontaneously with oxygen to form iron(III)oxide according to the following reaction: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) The reason this reaction is spontaneous
- For the following reaction: Fe (s) + BeO (aq) \to Be (s) + Fe_2O_3 (aq) a. Give the oxidation state of every atom in the following equation, b. State what is being oxidized and what is being reduced.
- Consider the following reaction and answer the following questions. 2Mg + O2 arrow 2MgO a. How many moles of oxygen gas are needed to react with 12.3 moles of magnesium? b. How many moles of magnesium are needed to react with 30.2 grams of O2?
- An excess of solid iron is reacted with 0.25 g MnCl4 according to the following reaction: MnCl4 (aq) + 2Fe(s) 2FeCl2(aq) + Mn(s) How many moles of solid manganese can be produced from the given amount of salt in the reaction above? Assume the salt is the
- What is the number of formula units in a 3.59 mol sample of FeCl3?
- CaO+CO2 yields CaCO3. What mass of CaO is needed, to absorb 22 grams of CO2, according to the balanced chemical equation above? (Molar masses: CaO=56g/mol, CO2=44g/mol)
- Give the equation for the reaction of FeCl3 + H2O2. Remember, FeCl3 is a catalyst.
- How many grams of O2 are needed to react with 8.85 g of ethanol? Express the mass to three significant figures and include the appropriate units.
- How many molecules of CuSO_4 are required to react with 2.0 moles Fe?
- Suppose 4,000 grams of heptane is combusted with 7,000 grams of oxygen. a. What is the limiting reactant? b. How much CO2 is produced? c. How much excess reactant is there?
- Assume 171 grams of diborane, B_2H_6, reacts with excess oxygen O_2. Determine the mass of boron oxide, B_2O_3, formed from this reaction. B_2H_6 (g) + 3O_2(g) \to B_2O_3 (s) + 3 H_2O(l) (Round molar masses to the hundredths place (0.01 g))
- What is the total number of grams of O2(g) needed to react completely with 0.50 moles of C2H2(g) for the balanced equation below? 2C2H2(g) + 5O2(g) arrow 4CO2(g) + 2H2O(g)
- To produce iron sulfide and hydrochloric acid, the reactants iron chloride and hydrogen sulfide react together. In this reaction, 100.0 g of iron (iii) chloride (FeCl3) reacts with 54 g hydrogen sulfide. What is the balanced equation for this?
- Given the following chemical equation: FeCl2 + 2NaOH arrow Fe(OH)2 + 2NaCl, A) If I start the chemical reaction with 3.51 moles of NaOH, how many moles of NaCl can I make? B) If I start the chemical reaction with 4.2 moles of FeCl2, how many moles of NaCl
- How many grams of oxygen are consumed when 18.0 L of CH4 gas react completely in the following equation? CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
- Consider the following reaction. FeCl2 + 2NaOH arrow Fe(OH)2 + 2NaCl If you start with 3.51 moles of NaOH, how many moles of NaCl can you make?
- Identify the limiting reactant and determine the mass of CO2 that can be produced from the reaction of 25.0g of C3H8 with 75.0g of O2 according to the following equation.
- Write the chemical equation for the word equation below and determine the type of reaction (synthesis combination, decomposition, single-displacement, double-displacement, or combustion). Iron plus octasulfur yields iron (II) sulfide
- Use the following reaction with fictional elements and compounds to answer the questions below: X_2Z_3 + A\to X + AZ_2 a) Balance the equation. What type of reaction is this? b) How many grams of A are needed to react with 7300 mg of X_2Z_3? c) How...
- 4Fe(s) + 3O_{2}(g) \rightarrow 2Fe_{2}O_{3}(s); change of H = -1652 kJ a. How much heat is released when 4.00 mol iron is reacted with excess O_{2}? b. How much heat is released when 1.00 mol Fe_{2}O_{3} is produced? c. How much heat is released when 1.00
- How many grams of CH4 are needed to react completely with 6.4 grams of O2? CH4 + O2 arrow CO2 + H2O
- For the reaction 2AgNO3 +NaCrO4 \rightarrow Ag2CrO4 +2NaNO3. How many grams of silver chromate are produced from 69.7g of silver nitrate?
- Calculate the molar mass for Mn2O3 , an oxide of manganese. Express your answer to five significant figures.
- What are stoichiometric reacting masses and limiting reactants? How to calculate stoichiometric reacting masses?
- According to the following reaction, how many moles of mercury will be formed upon the complete reaction of 23.2 grams of mercury(II) oxide? 2HgO(s) \to 2Hg(l) + O2(g)
- Explain the need for coefficients when balancing the following reaction. Al + Fe2O3 arrow Fe + Al2O3
- A) Calculate the number of moles of iron in a 15.0 g sample of iron. B) Calculate the number of atoms in 0.25 mol of silicon. C) Calculate the mass in grams needed to have 2.65 times 10^(22) atoms of calcium.
- How many moles of carbon dioxide are produced when 3.00 mol of oxygen react completely in the following equation? C_3H_8 + 5 O_2 rightarrow 3 CO_2 + 4 H_2O
- How many grams of chromium are needed to react with an excess of CuSO4 to produce 127.0g Cu? 2Cr(s)+3CuSO4(aq) yields Cr2(SO4)3(aq)+3Cu(s)
- Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is: S2(g) + C(s) arrow CS2(g); Kc = 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 13.7 mol S2(g) with excess carbon in a 6.25 L reaction vessel held at
- Consider the following reaction: I2O5 (g) + 5 CO (g) --> 5 CO2 (g) + I2 (a) 80.0 grams of Iodine (V) oxide reacts with 28.0 grams of carbon monoxide. Determine the mass of iodine which could be produc
- What volume of oxygen gas is required to react completely with 0.246 mol of carbon monoxide according to the following reaction at 0 C and 1 atm?CO (g) + O (g) \to CO_2 (g)
- Consider the following reaction: 4 PH3 + 8 O2 to P4O10 + 6 H2O a. How many grams of PH3 are required to react with 100 g of O2? b. How many grams of P4O10 are produced when 100 g of O2 react? c. How many moles of water are produced when 100 g of O2 react?
- Use dimensional analysis to solve the question below: "If you evaporated 250 mL of a 3.5 M solution of iron (ii) nitrite (Fe(NO2)2), what mass of iron (ii) nitrite would you recover?"
Explore our homework questions and answers library
Browse
by subject