Concept explainers
A 180.0-mg sample of an alloy of iron and metal X is treated with dilute sulfuric acid, liberating hydrogen and yielding Fe2+ and X3+ ions in solution. It is known that the alloy contains 20.0 percent iron by mass. The alloy yields 50.9 mL of hydrogen collected over water at 22°C and a total pressure of 750.0 torr. What is element X?
Interpretation:
The element X should be identified.
Concept introduction:
Ideal gas is the most usually used form of the ideal gas equation, which describes the relationship among the four variables P, V, n, and T. An ideal gas is a hypothetical sample of gas whose pressure-volume-temperature behavior is predicted accurately by the ideal gas equation.
Use the ideal gas equation,
Answer to Problem 11.110QP
The element with a molar mass of
Explanation of Solution
To calculate the total pressure of water and the pressure of Hydrogen in atm.
The partial pressure of water at
Solving for
Converting to atm
Given that
The total pressure is the sum of the partial pressures of the individual components in the mixture, in this case hydrogen and water.
The Hydrogen pressure was calculated, the pressure of water is subtracts from total pressure then we get the Hydrogen pressure is
The pressures in atm are calculated by plugging in the values of the given 1 torr and 1 Pa. The pressures in atm was found to be
To calculate the number of moles
The moles of
To calculate the number of moles
The moles of
Iron yields
Next, determine the amount of
The remaining moles of
Metal X yields
The balanced equation is:
Finally, using the mole ratio between X and H2, determine the number of moles of X needed to produce
Since there are 0.144 0g of metal X, the molar mass is:
The element with a molar mass of
The element X was identified.
Want to see more full solutions like this?
Chapter 11 Solutions
Loose Leaf For Chemistry: Atoms First With Connect 2y Access Card
- Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s)+O2(g)SO2(g)2SO2(g)+O2(g)2SO3(g) What volume of O2(g) at 350.C and a pressure of 5.25 atm is needed to completely convert 5.00 g sulfur to sulfur trioxide?arrow_forwardGiven that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardYou have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning