We have to calculate the number of carbon atoms present in 2-carat pure diamond.
The number of carbon atoms present in 2-carat pure diamond is: 0.19 X 10²³ number of carbon atom.
Diamond is one allotrope of carbon. Atomic mass of carbon is 12.
Mass of one mole carbon atom is 12 g. One mole carbon contains Avogadro's number i.e, 6.023 X 10²³ number of atoms.
0.40 g diamond contains 0.40/12 moles= 0.033 moles of carbon atom.
So, number of carbon atoms present in 0.40 g diamond (i.e, 0.033 mole diamond) is 0.033 X 6.023 X 10²³= 1.98 X 10²²=0.19 X 10²³ .
Therefore, 0.19 X 10²³ number of carbon atoms are in a 2-carat pure diamond that has a mass of 0.40 g
Gas is a substance that will not phase change.
And vapor is a substance above it's boiling point temperature.
In a redox reaction electrons are lost and gained in equal numbers. The species that is oxidized gives electrons to the species that is reduced. I hope this helps. Let me know if anything is unclear.
Okay
Mr (H2O)= 18g
therefore moles of H2O
is 720.8/18= 40.04mol
the ratio of H2 to O2 to H2O is
2 : 1 : 2
so moles of H2 is same as H2O here
H2= 40.04moles
moles of O2 is half
so 40.04 x 0.5
20.02moles
grams of O2 is
its moles into Mr of O2
that's 20.02 x 32 = 640.64g
The correct answer for the question that is being presented above is this one: "A. The accepted model of the atom was changed.<span>" </span>J J Thomson discovered the electrons and performed experiment using the cathode ray tube
Here are the following choices:
<span>A. The accepted model of the atom was changed.
B. The accepted model of the atom was supported.
C. Cathode ray tubes were no longer used in experiments due to poor results.
D. Cathode ray tubes became the only instrument of use in the study of atoms</span>
