Which of the following is more likely to represent the mass 6.022x10^23 atoms of hydrogen?

6.022x10^23 atoms of hydrogen = 1 mol H, and 1 mol of H * 1.008g/mol H = 1.01g "a" mass of H-atom =1.67 x 10^-24 g = 1.67 × 10^-27 kilograms =1 atomic mass unit (amu), "b"

a. 1.01g - 6.022*10^23 atoms of hydrogen represents Avogadro's number, which is called a mole and the theoretical amount of atoms in a mole of any element. 6.022*10^23 atoms hydrogen = 1 mole hydrogen = 1.01g hydrogen. The atomic weight of hydrogen from the periodic table is 1.01 amu which is also how much a mole of hydrogen weighs, 1.01g. This is true for every other element on the chart. Ex: 1 mole gold (Au) = 196.97g = 6.022*10^23 particles of gold, and so on, so 1.01g is more likely. b. 1.01 amu - An amu is an atomic mass unit or atomic weight and is approximately equal to the mass of one proton or one neutron. Since hydrogen is only one proton and one electron, one atom weighs approximately one amu, the electron's weight is 8.9278 x10^-30 and not figured into the atomic weight, so 1.01 amu is most likely.

atoms H = (6.02*10^23 atoms H) * (1 mol H / 6.02*10^23 atoms H) * (1 grams H / 1 mol H) = 1 grams H The answer is a. --------------------------------- Also, Which of the following is more likely to represent the mass of one atoms of hydrogen? mass of hydrogen atom = (1 atom H) * (1 amu / 1 atom H) = 1 amu The answer is b.

1: Hydrogen's formula weight is about 1 gram per mole. That means a mole of Hydrogen would equal about 1 gram. So, A 2: An atomic mass unit (amu) is used to measure subatomic particles. Since hydrogen only has one electron/proton/neutron, 1 amu would be appropriate. B.

6.023 x 10^23 is one mole of molecules. So if you have just ATOMS of H and not molecules of H (H2) then the answer is 1.01 g.

a. 1.01g - 6.022*10^23 atoms of hydrogen represents Avogadro's number, which is called a mole and the theoretical amount of atoms in a mole of any element. 6.022*10^23 atoms hydrogen = 1 mole hydrogen = 1.01g hydrogen. The atomic weight of hydrogen from the periodic table is 1.01 amu which is also how much a mole of hydrogen weighs, 1.01g. This is true for every other element on the chart. Ex: 1 mole gold (Au) = 196.97g = 6.022*10^23 particles of gold, and so on, so 1.01g is more likely. b. 1.01 amu - An amu is an atomic mass unit or atomic weight and is approximately equal to the mass of one proton or one neutron. Since hydrogen is only one proton and one electron, one atom weighs approximately one amu, the electron's weight is 8.9278 x10^-30 and not figured into the atomic weight, so 1.01 amu is most likely.

1: Hydrogen's formula weight is about 1 gram per mole. That means a mole of Hydrogen would equal about 1 gram. So, A 2: An atomic mass unit (amu) is used to measure subatomic particles. Since hydrogen only has one electron/proton/neutron, 1 amu would be appropriate. B.

atoms H = (6.02*10^23 atoms H) * (1 mol H / 6.02*10^23 atoms H) * (1 grams H / 1 mol H) = 1 grams H The answer is a. --------------------------------- Also, Which of the following is more likely to represent the mass of one atoms of hydrogen? mass of hydrogen atom = (1 atom H) * (1 amu / 1 atom H) = 1 amu The answer is b.

6.023 x 10^23 is one mole of molecules. So if you have just ATOMS of H and not molecules of H (H2) then the answer is 1.01 g.