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The density is 10.7 g/mL. The sample is not pure lead because the density of pure lead is 11.3 g/mL.
Mass and volume are extensive properties, which are dependent upon the size of the sample. A larger sample will have a greater mass and volume than a smaller sample. Density is an intensive property, which does not depend on the size of the sample. Density is a ratio of mass to volume, which does not vary with the size of the sample. The density of a larger sample will be the same as the density of a smaller sample.
Mass [g] (Ag)=(10.46g Ag/1cm Ag)(12.99cm Ag/1) The "centimeters" units cancel out to leave you with grams of Ag. Just multiply across: 12.99x10.46 for your answer, in grams.
Density = mass/volume To find mass when density and volume are known, multiply the density times the volume.
There is a thing called heavy water. It is pure water that has a deuterium in it known as D20 instead of H20. It is pure but does not have the same mass.
The volume and the mass of sample both depend on the size of the sample.A small sample has small volume and small mass, a big sample has big volumeand big mass. But the ratio of mass to volume is constant for a pure sample ofa substance, no matter what size the sample is. That ratio is called the densityof the substance.
The idea is to divide the mass by the volume.
The density is 10.7 g/mL. The sample is not pure lead because the density of pure lead is 11.3 g/mL.
Density = Mass/Volume so Volume = Mass/Density Vol = 0.25/3.5 = 0.071429 cubic cm
You know that the density of pure water is 1g/cm3. If you also know the volume of the water, you can multiply the two and get the mass.
Mass and volume are extensive properties, which are dependent upon the size of the sample. A larger sample will have a greater mass and volume than a smaller sample. Density is an intensive property, which does not depend on the size of the sample. Density is a ratio of mass to volume, which does not vary with the size of the sample. The density of a larger sample will be the same as the density of a smaller sample.
The definition doesn't require that level of complexity. Any physical sample of any solid, fluid, or gasmust have both mass and volume, and so the ratio must exist. Can you think of an exception ?As long as the sample is pure, the ratio should be independent of the size of the sample.
The atomic mass of B is 10.8Amount of B = mass of pure sample/molar mass = 31.78/10.8 = 2.94mol There are 2.94 moles of the element boron in a 31.78g pure sample.
Mass [g] (Ag)=(10.46g Ag/1cm Ag)(12.99cm Ag/1) The "centimeters" units cancel out to leave you with grams of Ag. Just multiply across: 12.99x10.46 for your answer, in grams.
12.99cm is not a volume
To determine the percentage of oxygen in FeCr2O4, you would first calculate the molar mass of the compound (iron(II) chromite) using the atomic masses of each element (Fe = 55.85 g/mol, Cr = 51.996 g/mol, O = 16 g/mol). Then, calculate the molar mass percentages of each element within the compound, and finally, determine the percentage of oxygen by mass in the compound.
No.