Concept explainers
Interpretation: The amount of water required in kilograms has to be calculated to get 2.0 L of
Concept introduction:
Ideal gas equation is given as follows,
Answer to Problem 25.12QP
The amount of water required to get 2.0 L of
Explanation of Solution
Capture the given data
Pressure is given as
Temperature is given as
Gas constant value is
The number of moles of deuterium is calculated by the use of modified ideal gas equation.
The number of moles of deuterium is 0.07357 moles.
By using the modified ideal gas equation and given data the number of moles of deuterium is calculated as 0.07357 moles.
To determine: The number of moles of water
The abundance of deuterium is given as 0.015 percent.
The number of moles of
By the use of calculated moles of deuterium and percent of deuterium the number of moles of water is calculated as
To determine: The amount of
Recovery is given as 80 percent. The amount of water needed is calculated as follows:
The amount of
By the use of moles of water and recovery of deuterium the amount of water is needed to produce 2.0 L of deuterium is calculated as 11.04495 Kg.
The required amount of water to produce the given amount of deuterium was calculated.
Want to see more full solutions like this?
Chapter 25 Solutions
Chemistry: Atoms First
- Why does white phosphorus consist of tetrahedral P4 molecules while nitrogen consists of diatomic N2 molecules?arrow_forwardWhat mass of CaH2 is necessary to react with water to provide enough hydrogen gas to fill a balloon at 20 C and 0.8 arm pressure with a volume of 4.5 L? The balanced equation is: CaH2(s)+2H2O(l)Ca(OH)2(aq)+2H2(g)arrow_forwardWhat is the most important commercial means of producing oxygen?arrow_forward
- The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine, because the reaction goes to completion. The amount of iodine produced is then determined by titration with sodium thiosulfate, Na2S2O3, which is oxidized to sodium tetrathionate, Na2S4O6. Potassium iodide was added in excess to 5.00 mL of bleach (density = 1.00 g/mL). This solution, containing the iodine released in the reaction, was titrated with 0.100 M Na2S2O3. If 34.6 mL of sodium thiosulfate was required to reach the endpoint (detected by disappearance of the blue color of the starch iodine complex), what was the mass percentage of NaClO in the bleach?arrow_forwardXenon trioxide, XeO3, is reduced to xenon in acidic solution by iodide ion. Iodide ion is oxidized to iodine, I2. Write a balanced chemical equation for the reaction.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning