A technique once used by geologists to measure the density of a mineral is to mix twodense liquids in such proportions that the mineral grains just float. When a sample of the mixture in which the mineral calcite just floats is put in a special density bottle, the weight is 15.4448 g. When empty, the bottle weighs 12.4631 g, and when filled with water, it weighs 13.5441 g. What is the densityof the calcite sample? (All measurements were carried out at 25 °C, and the density of water at 25 °C is 0.9970 g/mL. ) At the left, grans of the mineral calcite float the surface of the liquidbromoform ( d = 2.890 g / m L ) . At the right, the grains sink to thebottom of chloroform ( d = 1.444 g / m L ) . By mixing bromoform and chloroform in just the proportions required so that the grains barely float, the density of the calcite be determined (Exercise 62).
A technique once used by geologists to measure the density of a mineral is to mix twodense liquids in such proportions that the mineral grains just float. When a sample of the mixture in which the mineral calcite just floats is put in a special density bottle, the weight is 15.4448 g. When empty, the bottle weighs 12.4631 g, and when filled with water, it weighs 13.5441 g. What is the densityof the calcite sample? (All measurements were carried out at 25 °C, and the density of water at 25 °C is 0.9970 g/mL. ) At the left, grans of the mineral calcite float the surface of the liquidbromoform ( d = 2.890 g / m L ) . At the right, the grains sink to thebottom of chloroform ( d = 1.444 g / m L ) . By mixing bromoform and chloroform in just the proportions required so that the grains barely float, the density of the calcite be determined (Exercise 62).
A technique once used by geologists to measure the density of a mineral is to mix twodense liquids in such proportions that the mineral grains just float. When a sample of the mixture in which the mineral calcite just floats is put in a special density bottle, the weight is 15.4448 g. When empty, the bottle weighs 12.4631 g, and when filled with water, it weighs 13.5441 g. What is the densityof the calcite sample? (All measurements were carried out at 25 °C, and the density of water at 25 °C is 0.9970 g/mL. )
At the left, grans of the mineral calcite float the surface of the liquidbromoform
(
d
=
2.890
g
/
m
L
)
. At the right, the grains sink to thebottom of chloroform
(
d
=
1.444
g
/
m
L
)
. By mixing bromoform and chloroform in just the proportions required so that the grains barely float, the density of the calcite be determined (Exercise 62).
A flask has a mass of 78.23 g when empty and 593.63 g when filled with water. When the same flask is filled with concentrated sulfuric acid, H2SO4, its mass is 1026.57 g. What is the density of concentrated sulfuric acid?
Crime scene investigators keep a wide variety of compounds on hand to help with identifying unknown substances they find in the course of their duties. One such investigator, while reorganizing their shelves, has mixed up several small vials and is unsure about the identity of a certain powder. Elemental analysis of the compound reveals that it is 67.31 % carbon, 6.978% hydrogen, 4.617% nitrogen, and 21.10% oxygen by mass.
Which of the compounds could the powder be?
C17H19NO3C17H19NO3 = morphine, analgesic
C17H21NO4C17H21NO4 = cocaine, illicit drug
C7H5N3O6C7H5N3O6 = 2,4,6-trinitrotoluene (TNT), commonly used explosive
C10H15NC10H15N = methamphetamine, stimulant
C4H5N2OC4H5N2O = caffeine, stimulant
C11H15NO2C11H15NO2 = 3,4-methylenedioxymethamphetamine (MDMA), illicit drug
C21H23NO5C21H23NO5 = heroin, illicit drug
C3H6NO3C3H6NO3 = hexamethylene triperoxide diamine (HMTD), commonly used explosive
2. The picture in the introduction shows that the mass of a crucible and lid was
determined to be 22.1504 g. The hydrate was placed into the crucible, and now
the crucible with lid and hydrate weighed 24.2901 g. The hydrate in the crucible
was then heated and all water was removed. Once cooled, the crucible with lid
and dried hydrate weighed 23.0063 g.
a) Calculate the mass of the hydrate.
b) Calculated the mass of water lost.
c) Calculate the mass percentage of water in the hydrate.
percent (%)
composition =
of water
mass of water lost
х 100
mass of entire hydrate
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.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
The Creation of Chemistry - The Fundamental Laws: Crash Course Chemistry #3; Author: Crash Course;https://www.youtube.com/watch?v=QiiyvzZBKT8;License: Standard YouTube License, CC-BY