Consider two samples of carbon. One is a sample of one mole of carbon atoms obtained from the environment (i.e. isotopes are pre
sent according to their natural abundance), and the other is a sample of one mole of carbon-12 atoms (i.e. isotopically pure). Which sample has a higher mass, or are they both the same mass? Justify your answer, either with words or mathematically
The sample obtained from the environment has a higher mass
Explanation:
A simple way to put the answer is that the element carbon -as found in nature- has a molar mass of 12.0107 g/mol, because there are a few isotopes of 14C and 13C; and <em>the molar mass is an expression of the isotopes' natural abundance</em>.
So 1 mole of carbon obtained from the environment would weigh 12.0107 g, while a sample of isotopically pure carbon would weigh 12.0000 g.
First you have to moles so multiply .0483L X .55M= .026565 Multiply moles by mole ratio which is 1/2, so the moles becomes .013283 now molarity=moles/volume; divide .013283/.015L=.885533M significant figures and you final answer is 0.89M
