Concept explainers
In the thermite reaction, iron(III) oxide is reduced by aluminum to give molten iron
Fe2O3(S) + 2 Al(S) → 2 Fe(l) + Al2O3(S)
If you begin with 10.0 g of Fe2O3 and 20.0 g of AI,
- (a) Which reactant is limiting?
- (b) What mass of Fe can be produced?
- (c) What mass of the excess reactant remains after the limiting reactant is consumed?
- (d) Set up an amounts table for this problem.
(a)
Interpretation:
The limiting reactant of the reaction has to be identified.
Concept introduction:
Limiting reagent: limiting reagent is a reactant, which consumes completely in the chemical reaction. The quantity of the product depends on this limiting reagent, it can be determined with the help of balanced chemical equation for the reaction.
Answer to Problem 17PS
Explanation of Solution
Balanced chemical equation for the given reaction is,
To find the mass of product formed in the reaction, the amount of each reactant involved in the given reaction should be determined.
Therefore,
The mass of
The amount of
Therefore, the reactant
(b)
Interpretation:
Mass of Fe produced in the reaction has to be determined.
Concept Introduction:
- The number of moles of any substance can be determined using the equation,
- The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
- For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
- Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
Answer to Problem 17PS
The maximum mass of
Explanation of Solution
From the previous calculation, the amount of
The mass of
The maximum mass of
(c)
Interpretation:
Mass of excess reactant remains after the consumption of limiting reactant has to be calculated.
Answer to Problem 17PS
The excess mass of the reactant remains after the limiting reactant is consumed is
Explanation of Solution
The mass of Al remains when all the
Reaction began with
(d)
Interpretation:
Amount table for the given problem has to be set up.
Explanation of Solution
The results of the above calculations can be summarized in an amounts table as follows,
Equation | ||||
Initial amount (mol) |
|
|
0 |
0 |
Change in amount upon reaction (mol) |
|
|
|
|
Amount after complete reaction (mol) |
0 |
|
|
|
Want to see more full solutions like this?
Chapter 4 Solutions
Chemistry & Chemical Reactivity
- 4.24 Ammonia gas can be prepared by the reaction CaO(s)+2NH4Cl(s)2NH3(g)+H2O(g)+CaCl2(s) If 112 g of CaO reacts with 224 g of NH4Cl, how many moles of reactants and products are there when the reaction is complete?arrow_forward4.69 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. 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.arrow_forward4.108 Elemental analysis is sometimes carried out by combustion of the sample. For a hydrocarbon, the only products formed are CO2 and H2O. If a 1.36-g sample of an unknown hydrocarbon is burned and 2.21 g of H2O is produced along with 4.07 g of CO2, what is the empirical formula of the hydrocarbon?arrow_forward
- Tungsten (W) metal, which is used to make incandescent bulb filaments, is produced by the reaction WO3+3H23H2O+W How many grams of H2 are needed to produce 1.00 g of W?arrow_forwardYou take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.arrow_forwardPhosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water. 14P4O10(s)+32H2O(l)H3PO4(aq);H=96.2kJ What is H for the reaction involving 1 mol of P4O10? P4O10(s)+6H2O(l)4H3PO4(aq)arrow_forward
- Bacterial digestion is an economical method of sewage treatment. The reaction is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate ions. What mass of bacterial tissue is produced in a treatment plant for every 1.0 104 kg of wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium ions are consumed by the bacteria.arrow_forwardHow many grams of beryllium (Be) are needed to react completely with 45.0 g of nitrogen (N2) in the synthesisof Be3N2?arrow_forwardThe active ingredient in some antiperspirants is aluminum chlorohydrate, Al2(OH)5Cl. Analysis of a 2.000-g sample of antiperspirant yields 0.334 g of aluminum. What percent (by mass) of aluminum chlorohydrate is present in the antiperspirant? (Assume that there are no other compounds containing aluminum in the antiperspirant.)arrow_forward
- 4.16 Many metals react with halogens to give metal halides. For example, iron reacts with chlorine to give iron(II) chloride, FeCl2: Fe(s)+Cl2(g)FeCl2(s) Beginning with 10.0 g iron, what mass of Cl2, in grams, is required for complete reaction? What quantity of FeCl2, in motes and in grams, is expected?arrow_forwardNitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2 mol NO, calculate how many moles and how many grams of O2 are required for complete reaction. Calculate what mass of NO2, in grams, is produced.arrow_forwardA titanium ore contains rutile (TiO2) plus some iron oxide and silica. When it is heated with carbon in the presence of chlorine, titanium tetrachloride, TiCl4, is formed. TiO2(s)+C(s)+2Cl2(g)TiCl4(g)+CO2(g) Titanium tetrachloride, a liquid, can be distilled from the mixture. If 35.4 g of titanium tetrachloride is recovered from 18.1 g of crude ore, what is the mass percentage of TiO2 in the ore (assuming all TiO2 reacts)?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning