A. The number of particles in exactly one gram of pure substance
B. The amount of substance that contains the same mass as the mass of 12 grams of carbon-12
C. The amount of substance that contains the same volume as the volume of 12 grams of carbon-12
D. The amount of substance that contains as many particles as there are atoms in 12 grams of carbon-12
B. The amount of substance that contains the same mass as the mass of 12 grams of carbon-12
C. The amount of substance that contains the same volume as the volume of 12 grams of carbon-12
D. The amount of substance that contains as many particles as there are atoms in 12 grams of carbon-12
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D
Are you asking all your homework or exam questions? I've now answered question 14 and question 8. Maybe you should study more.
Are you asking all your homework or exam questions? I've now answered question 14 and question 8. Maybe you should study more.
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The fact you have to ask this question tells me you need to review the concept of a mole.
For starters, there is Avogadro's number, abbreviated N or sometimes l (lower-case L). Avogadro's number is 6.022 x 10^23. A mole of any substance (either electrons, atoms or molecules) contains 6.022 x 10^23 particles. This convention allows chemists to convert (back and forth) between thinking about how many particles are involved (as in a chemical formula) and the mass of a particular substance in grams (as in weighing practical quantities of various substances.) ...and, as John W has reminded us, a mole of gas molecules occupies 22.4 liters at standard temperature and pressure. Nevertheless, the correct answer is D.
You need to remember that a mole of any substance weighs the same as its atomic mass in grams -- that a mole is one gram-atomic weight. If we had one mole of carbon-12 it would weigh exactly 12 grams and would contain 6.022 x 10^23 atoms of carbon-12. If we had one mole of helium it would weigh 4.0026 grams, would also have 6.022 x 10^23 atoms of helium of various isotopes, and would occupy 22.4 liters at STP.
The mole is an essential concept that will dog you for as long as you study chemistry. I suggest you keep at it until you really, really get it.
For starters, there is Avogadro's number, abbreviated N or sometimes l (lower-case L). Avogadro's number is 6.022 x 10^23. A mole of any substance (either electrons, atoms or molecules) contains 6.022 x 10^23 particles. This convention allows chemists to convert (back and forth) between thinking about how many particles are involved (as in a chemical formula) and the mass of a particular substance in grams (as in weighing practical quantities of various substances.) ...and, as John W has reminded us, a mole of gas molecules occupies 22.4 liters at standard temperature and pressure. Nevertheless, the correct answer is D.
You need to remember that a mole of any substance weighs the same as its atomic mass in grams -- that a mole is one gram-atomic weight. If we had one mole of carbon-12 it would weigh exactly 12 grams and would contain 6.022 x 10^23 atoms of carbon-12. If we had one mole of helium it would weigh 4.0026 grams, would also have 6.022 x 10^23 atoms of helium of various isotopes, and would occupy 22.4 liters at STP.
The mole is an essential concept that will dog you for as long as you study chemistry. I suggest you keep at it until you really, really get it.
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B.
Also, 22.4 L of any gas at STP contains one mole of molecules.
Also is the number of particles in 6.022x10^23 particles of the substance.
Also having one gram-molecular mass of a substance.
Also, 22.4 L of any gas at STP contains one mole of molecules.
Also is the number of particles in 6.022x10^23 particles of the substance.
Also having one gram-molecular mass of a substance.