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What approximate mass would a sample of naturally occurring boron (B) that contains 1 and times 106 atoms of boron have?
The molar mass of boron is approximately 10.81 g/mol. To calculate the mass of 1 x 10^6 boron atoms, you divide 6.022 x 10^23 (Avogadro's number) by 1 x 10^6 to find the number of moles, which equals 0.001673 moles. Multiply this by the molar mass of boron to get approximately 0.0181 grams.
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What approximate mass would a sample of naturally occurring boron (B) that contains 1 x 106 atoms of boron have?
The molar mass of boron is approximately 10.81 g/mol. To find the mass of 1 x 10^6 atoms of boron, divide the number of atoms by Avogadro's number to get the number of moles, then multiply by the molar mass of boron. Therefore, the mass of 1 x 10^6 boron atoms would be approximately 1 x 10^-5 grams.
Which sample contains the greatest number of atoms a sample of Mn that contains 3.29E plus 24 atoms or a 5.18 mole sample of you?
Which sample contains the greatest number of atoms. A sample of Mn that contains 3.29E+24 atoms or a 5.18 mole sample of I?The sample of _____ contains the greatest number of atoms.Answer:In order to compare the two samples, it is necessary to express both quantities in the same units. Since the question was phrased in terms of atoms, it is convenient to convert moles of I to atoms of I.The conversion factor between atoms and moles is Avogadro's number: 6.02 x 1023 "things" / molTo convert 5.18 moles of I to atoms of I:atoms I= 5.18 mol I6.02 x 1023 atoms I = 3.12E+24 atoms I1 mol IMultiply by atoms per mole. Moles cancel out.The sample of Mn contains 3.29E+24 atoms.Since 3.12E+24 is smaller than 3.29E+24, the sample of Mn contains the greatest number of atoms.
How many atoms of 124Sn are present in 12.0 g of naturally occurring tin?
To determine the number of atoms of 124Sn in 12.0 g of naturally occurring tin, you need to first calculate the moles of tin using its molar mass (118.71 g/mol). Then, since natural tin consists of about 5% of 124Sn isotope, you can determine the number of moles of 124Sn in the sample. Finally, use Avogadro's number (6.022 x 10^23) to find the number of atoms of 124Sn.
What is the result when you total the individual percent abundance of isotopes of a given element?
How do you calculate percent abundance of an isotope?You find the isotope number and then you calculate that into a fraction and then turn the fraction into a percentage and divide it by the atomic number then times it by the mass and turn that answer into a percent and voila, there you have it.
Which sample of water contains the most heat energy 10 g at 10 degreescelsius or 20 g at 10 degrees celsius?
The sample of water that contains the most heat energy is the 20 g sample at 10 degrees Celsius because it has double the mass of the 10 g sample. Heat energy is directly proportional to mass, so the sample with more mass will contain more heat energy.
What approximate mass would a sample of naturally occurring boron B that contains?
The atomic weight of boron (B) is approximately 10.81 g/mol. To calculate the mass contained in a sample, you need to know the number of moles present and then multiply that by the molar mass of boron.
How might you identify whether a mineral sample might be lodestone?
One way to identify if a mineral sample might be lodestone is through its magnetic properties. Lodestone is a naturally occurring magnet, so it will attract materials like iron. You can test this by seeing if the sample is attracted to a magnet. Additionally, lodestone is typically a form of magnetite, so if the sample looks similar to magnetite in appearance, it could be lodestone.
What approximate mass would a sample of naturally occurring boron (B) that contains 1 x 106 atoms of boron have?
The molar mass of boron is approximately 10.81 g/mol. To find the mass of 1 x 10^6 atoms of boron, divide the number of atoms by Avogadro's number to get the number of moles, then multiply by the molar mass of boron. Therefore, the mass of 1 x 10^6 boron atoms would be approximately 1 x 10^-5 grams.
What is the density of palladium 106?
Palladium consists of several isotopes. The density of a naturally occurring sample, which is a mixture of isotopes is 12.02 g/cm3. I have no reference material for individual isotopes. There is a book called the CRC Handbook of Chemistry and Physics which may have this information.
What song did biggie sample for nasty boy?
Contains a sample of "Cavern" by Liquid Liquid
Which air sample contains the most carbon dioxide?
the leg
The atomic mass of element A is 63.6 atomic mass units The only naturally occurring isotopes of element A are A-63 and A-65 The percent abundances in a naturally occurring sample of element A are clo?
69% A-63 and 31% A-65 is the answer. you can use these two references to try and help you.http://answers.yahoo.com/question/index?qid=20071024200207AAJx04whttp://answers.yahoo.com/question/index?qid=20070610034300AAadbfngood luck :)
What is an atom mass of an element?
The atomic mass of an element is the weight of the constituent atomic paraticles in an atom of a given isotope. The atomic weight is the weighted average mass for atoms in a naturally occurring sample of the element.Almost all of an atom's mass is found in the nucleus, consisting of protons and neutrons.
What is an atomic mass of an element?
The atomic mass of an element is the weight of the constituent atomic paraticles in an atom of a given isotope. The atomic weight is the weighted average mass for atoms in a naturally occurring sample of the element.Almost all of an atom's mass is found in the nucleus, consisting of protons and neutrons.
What atomic mass of an element is?
The atomic mass of an element is the weight of the constituent atomic paraticles in an atom of a given isotope. The atomic weight is the weighted average mass for atoms in a naturally occurring sample of the element.Almost all of an atom's mass is found in the nucleus, consisting of protons and neutrons.
What is the atomic mass is an element?
The atomic mass of an element is the weight of the constituent atomic paraticles in an atom of a given isotope. The atomic weight is the weighted average mass for atoms in a naturally occurring sample of the element.Almost all of an atom's mass is found in the nucleus, consisting of protons and neutrons.
A sample of ascorbic acid contains 1.50 of carbon and 2.00 of oxygen while another sample of ascorbic acid contains 6.35 of c. How many grams of oxygen does it contain?
23
