Concept explainers
Interpretation:
The mass of water produced when
Concept introduction:
Answer to Problem 66E
The mass of water produced when
Explanation of Solution
The reaction is given below.
The balanced equation for the reaction is given below.
In the reaction,
Therefore, the mole ratio is given below.
The mole ratio to obtain moles of
The molar mass of aluminum is
The molar mass of hydrogen is
The molar mass of oxygen is
Therefore, the molar mass of
The formula to calculate the moles of
The mass of
Substitute the molar mass and mass of
The formula to calculate the moles of
Substitute the value of moles of
In the reaction,
Therefore, the mole ratio is given below.
The mole ratio to obtain moles of
The molar mass of hydrogen is
The molar mass of oxygen is
The molar mass of sulfur is
Therefore, the molar mass of
The formula to calculate the moles of
The mass of
Substitute the molar mass and mass of
The formula to calculate the moles of
Substitute the value of moles of
Since,
The number of moles of
The molar mass of hydrogen is
The molar mass of oxygen is
Therefore, the molar mass of
The formula to calculate the mass of
The moles of
The molar mass of
Substitute the molar mass and moles of
Therefore, the mass of water produced when
The mass of water produced when
Want to see more full solutions like this?
Chapter 9 Solutions
Modified Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used. (a) Mg(OH)2(s)+HCl4(aq) (b) SO3(g)+H2O(l) (assume an excess of water and that the product dissolves) (c) SrO(s)+H2SO4(l)arrow_forwardOne of relatively few reactions that takes place directly between two solids at room temperature is Ba(OH)2+8H2O(s)+NH4SCN(s)Ba(SCN)2(s)+H2O(l)+NH3(g) In this equation, the 8H2O in Ba(OH)2 8H2O indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate. a. Balance the equation. b. What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?arrow_forwardWhen organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2formed can be determined by the reaction with hydrogen peroxide: H2O2(aq)+SO2(g)H2SO4(aq) The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1 .302-g sample of coal is burned, and the SO2is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000 M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.arrow_forward
- 4.49 Small quantities of hydrogen gas can be prepared by the following reaction: Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) How many grams of H2 can be prepared from 25.0 mL of 6.00 M H2SO4 and excess zinc?arrow_forwardNitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.arrow_forwardThe US Environmental Protection Agency (EPA) places limits on the quantities of toxic substances that may be discharged into the sewer system. Limits have been established for a variety of substances, including hexavalent chromium, which is limited to 0.50 mg/L. If an industry is discharging hexavalent chromium as potassium dichromate (K2Cr2O7), what is the maximum permissible molarity of that substance?arrow_forward
- What is the difference between a solute and a solvent?arrow_forwardWhat volume of 0.08892 M HNO3 is required to react completely with 0.2352 g of potassium hydrogen phosphate? 2HNO2(aq)+K2HPO4(aq)H2PO4(aq)+2KNO3(aq)arrow_forwardConsider the iron alloy described in Question 19. Suppose it is desired to prepare 1.00 kg of this alloy, what mass of each component would be necessary?arrow_forward
- What volume of 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s)+H2SO4(l)HCl(g)+NaHSO4(s)arrow_forwardWhen organic compounds containing sulfur are burned, sulfurdioxide is produced. The amount of SO2 formed can be determined by the reaction with hydrogen peroxide: H2O2(aq)+SO2(g)H2SO4(aq) The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.302-g sample of coal is burned and the SO2 is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000-M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning