2Fe,0, + 30 –→ 4Fe + 3CO2 When 9.20 moles of carbon dioxide are produced from the reaction above, how many moles of Iron(III) Oxide must have been present before the reaction took place? O 2.00mol Fe2O3 O 13.8mol Fe2O3 O 6.13mol Fe2O3 O 27.6mol Fe203

2Fe,0, + 30 –→ 4Fe + 3CO2 When 9.20 moles of carbon dioxide are produced from the reaction above, how many moles of Iron(III) Oxide must have been present before the reaction took place? O 2.00mol Fe2O3 O 13.8mol Fe2O3 O 6.13mol Fe2O3 O 27.6mol Fe203

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section: Chapter Questions

Problem 72AP

See similar textbooks

Related questions

Q: For the reaction: N2(g)+3H2(g)=2NH3(g), a sample contains 4 N2 molecules and 14H2 molecules. When…

A: Limiting reagent can be defined as the species which get completely consumed in the reaction and…

Q: 4 NH3 (g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (1I) When 8 moles of NH3 was used in a reaction, how many…

Q: What is the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00…

A: Given, 4.00 moles of C8H18 4.00 moles of O2

Q: how many moles of NH3 will be required to produce 10.9 moles of water?

A: Given :- 4NH3 + 7O2 →4NO2 + 6H2O Number of moles of H2O produced = 10.9 mol To be…

Q: Each molecular diagram represents an initial mixture of thereactants. How many molecules of Cl2 are…

A: From figure (a) Moles of HCl = 7 Moles of O2 = 1 From figure (b) Moles of HCl = 6 Moles of O2 = 3…

Q: x N2(g) + y H2(g) → z NH3 Which of the followings about the given reaction is wrong? (N:14 g/mol, H:…

Q: The combustion of propane may be described by the chemical equation C,H3 (g) + 5 0,(g) → 3 Co,(g) +…

A: Given,Mass of C3H8 = 95.3 gMoles of C3H8 can be calculated as:

Q: Consider the reaction below: N2 (g) + H2 (g) --> NH3 How many grams of NH3 will be produced if 1.5…

A: Given chemical reaction : N2 + 3 H2 ---> 2 NH3 Mass of N2 = ?

Q: Potassium chlorate decomposes upon slight heating in the presence of a catalyst according to the…

A: Given;

Q: 2Fe,0, + 30 → 4Fe + 3CO, When 9.20 moles of carbon dioxide are produced from the reaction above, how…

A: The answer to the following question is-

Q: The balanced equation P.(s) + 6 H2(g) --> 4 PH3(g) tells us that 7.0 mol H, * O reacts with 3.5 mol…

Q: how many grams of bromine are required to completely react 0.557 grams of aluminum

A: Given :- 2Al + 3 Br2 ---------> 2AlBr3 Mass of Al = 0.557 g To calculate :- mass of Br2…

Q: 48. For the reaction shown, find the limiting reactant for each of the initial quantities of…

Q: 7. Aluminum metal weighing 2.82 g is exposed to 2.56 g oxygen gas to produce aluminum oxide. (Molar…

Q: If 24.1 g of NO and 13.8 g of O, are used to form NO, how many moles of excess reactant will be left…

A: Given, 2 NO (g) + O2 (g) ➝ 2 NO2 (g) Mass of NO = 24.1 g Mass of O2 = 13.8 g Moles of excess…

Q: Salicylic acid reacts with acetic anhydride to form aspirin, acetylsalicylic acid. If the percent…

A: Salicylic acid reacts with acetic anhydride to form aspirin and water. The equation for the balanced…

Q: 14. When nonane (C9H20) is burned in oxygen gas, what is the sum of the coefficients in the properly…

A: Since when we burn any hydrocarbon, we get carbon dioxide and water as products. hence the reaction…

Q: 5 F.(g) + 2 NH3(g) → N¿F«(g) + 6 HF(g) a) How many grams of HF will form when 57 grams of F2 reacts…

Q: In the balanced reaction, CH4 + 2 O2 CO2 + 2 H20, how many moles of CO2 will be produced when 0.50…

Q: A reaction mixture initially contains 0.25 moles of ZnS and 0.25 moles of O2. After the reaction is…

Q: Consider the following two-step reaction sequence. 2HCI + CaCO3 → CaCl2 + CO2 + H2O 2NazPO4 + 3CaCl2…

Q: Which of the balanced chemical equations is consistent with the following pictorial representation…

Q: You mix 54.26 g methane (CH4) gas and 74.25 g oxygen gas and ignite the mixture. A bright flash and…

A: Given: Mass of CH4 taken = 54.26 g. And mass of O2 taken = 74.25 g.

Q: Determine the theoretical yield of alum (KAl(SO4)2·12 H2O), in units of g, if a student starts with…

A: Interpretation: The theoretical yield of alum in grams is to be determined. Given: Theoretical yield…

Q: Calcium oxide (CaO) reacts with tetraphosphorus decoxide (P4010) to form calcium phosphate (Ca3…

A: Number of moles can be calculated by dividing the given mass with molecular mass.

Q: Consider the reaction below. 2Al2O3 ---> 4Al + 3O2 How many moles of oxygen are produced if 11.0…

Q: 3. What mass of HgO is required to produce 0.692 mol of O2? 2 HgO(s) → 2 Hg(ℓ) + O2(g)

Q: Each step of a four-step reaction has a yield of 75.00%. What is the percent yield for the overall…

A: The given reaction takes place in four steps. In the first step, the reaction yield is 75%.

Q: An important reaction sequence in the industrial production of nitric acid is the following: N2(g) +…

Q: How many moles of O2 would be required to generate 13.0 mol of NO2 in the reaction below assuming…

A: The given reaction is, Actual mass of NO2 formed is calculated as follows,

Q: The following are unbalanced equations. They show the kinds of reactants and products involved but…

A: (a) The given reaction is, Here, HgO decomposed to Hg and O2. Hence, the reaction is decomposition.…

Q: Consider the reaction between ammonium and oxygen: 4 NH3 ) + 5 02 (e) --> 4 NO () + 6 H20 ) A…

A: In this question answer does not matched any of the above option.The answer of this question should…

Q: What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of…

A: Percent yield =To be determined Experimental Yield = 28.16 gTheoretical Yield = 112.7 g

Q: Ether, (C2H5)2O, which was originally used as an anesthetic but has been replaced by safer and more…

A: Moles=given massmolar massGiven,If 19.7 g C2H5OHreacts with excess H2SO4Molar mass of Ethanol,…

Q: 18. Metal hydrides react with water to form hydrogen gas and the metal hydroxide such as in the…

Q: Determine the percent yield of a reaction that produces 18.65 g of Fe when 35.00 g of Fe,03 react…

Q: For the reaction, compute the theoretical yield of the product in moles for each of the following…

A: a. Theoretical yield of product is 1.0 mole.

Q: If 0.0916 g P406 is mixed with O.113 g H2O, what is the theoretical yield? P406+6H20 → 4H3 PO 3…

A: Given balanced reaction is : P4O6 + 6H2O --------> 4H3PO3 Mass of P4O6 = 0.0916 g Mass of H2O…

Q: Sodium metal reacts with water to form aqueous sodium hydroxide and hydrogen gas. Which equation…

A: Given : Reactants - 1) Sodium metal i.e Na 2) water i.e H2O Products - 1) Sodium…

Q: The following are unbalanced equations. They show the kinds of reactants and products involved but…

A: Disclaimer “Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: Milk of magnesia, which is an aqueous suspension of magnesium hydroxide, is used as an antacid in…

A: Given data: 28.68 g of MgCl₂ The balanced reaction is given as follows: Mg(OH)₂(s) + 2 HCl(aq) →…

Q: Consider the formation of lithium nitride from lithium and nitrogen: 6 Li + N2 ➜ 2 Li3N What is the…

Q: What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of…

A: The percent yield of a reaction can be calculated as follows: For the given reaction: The actual…

Q: A student was able to detect a mas O2. Oxygen was present in excess yield of the reaction? O 50.0% O…

Q: 100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow. MnO2 + 4…

A: A limiting reactant is the compound on the reactant side, which consumed completely during the…

Q: CacO316) - CaOe) + CO2(E) The theoretical yield for Cao in the reaction above is 18.9 g. What is the…

A: Find the solution below

Q: Consider the following reaction: CH4 (8) + O2 (g) → CO2 (8) + H2O (1) Hint- is this reaction…

A: Given: The unbalanced equation: CH4 (g) + O2 → CO2 (g) + H2O (l) The mass of CH4 produced = 5.0 g…

Q: If 21.7 g of NO and 13.8 g of O, are used to form NO, how many moles of excess reactant will be left…

Q: The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the…

A: Using mass-mass analysis on balanced reaction and formula of percentage yield we can solve this…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

2Fe,0, + 30 –→ 4Fe + 3C0,
When 9.20 moles of carbon dioxide are produced
from the reaction above, how many moles of Iron(III)
Oxide must have been present before the reaction
took place?
O 2.00mol Fe203
O 13.8mol Fe203
O 6.13mol Fe2O3
O 27.6mol Fe203

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Final answer

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Baking powder is a mixture of cream of tartar (KHC4H4O6)and baking soda (NaHCO3). When it is placed in an oven at typical baking temperatures (as part of a cake, ¡or example), it under goes the following reaction ( CO2makes the cake rise): msp;(KHC4H4O6)(s)+NaHCO3(s)KNaC4H4O6(s)+H2O(g)+CO2(g) u decide to make a cake one clay, and the recipe calls for baking powder. Unfortunately, you have no baking powder. You do have cream of tartar and baking soda, so you use stoichiometry to figure out how much of each to mix. the following choices, which is the best way to make baking powder? The amounts given in the choices are in teaspoons (that is, you will use a teaspoon to measure the baking soda and cream of tartar). Justify your choice. sume a teaspoon of cream of tartar has the same mass as a teaspoon of baking soda. l type='a'> Add equal amounts of baking soda and cream of tartar. i>Add a bit more than twice as much cream of tartar as baking soda. i>Add a hit more than twice as much baking soda as cream of tartar. i>Add more cream of tartar than baking soda, hut not quite twice as much. i>Add more baking soda than cream of tartar, hut not quite twice as much.
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?
Give the balanced equation for each of the following chemical reactions: a. Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor. b. Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate (NH4SCN).
4-55 For the reaction: (a) How many moles of N2 are required to react completely with 1 mole of O2? (b) How many moles of N2O3 are produced from the complete reaction of 1 mole of O2? (c) How many moles of O2 are required to produce 8 moles of N2O3?
A natural brine found in Arkansas has a bromide ion concentration of 5.00 × 10−3 M. If 210. g Cl2 were added to 1.00 × 103 L of the brine, determine the limiting reactant. calculate the theoretical yield of Br2 (d = 3.12 g/mL).
3.90 Pyrrole has the molecular formula C4H5N. When pyrrole reacts with O2, the products are CO2, H2O, and N2. Write a balanced equation for this reaction.
For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.107 Existing stockpiles of the refrigerant Freon-12, CF2Cl2 must be destroyed under the terms of the Montreal Protocol because of their potential for banning the ozone layer. One method for doing this involves reaction with sodium oxalate: CF 2 Cl 2 + 2Na 2 C 2 O 4 2NaF+2NaCl+C+ 4CO 2 S If you had 150 tons of Freon-12, describe how you would know how much sodium oxalate you would need to make that conversion. Freon-12, CF2Cl2
Black smokers are found in the depths of the oceans. Thinking that the conditions in these smokers might be conducive to the formation of organic compounds, two chemists in Germany found the following reaction could occur in similar conditions. 2 CH3SH + CO CH3COSCH3 + H2S If you begin with 10.0 g of CH3SH and excess CO, (a) What is the theoretical yield of CH3COSCH3? (b) If 8.65 g of CH3COSCH3 is isolated, what is its percent yield?
4.68 The pictures below show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (Green balls represent B atoms and orange balls are A atoms). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Explain how an equation can be balanced even if the number of reactant particles differs from the number of product particles.