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guajiro [1.7K]
3 years ago
6

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
Chemistry
1 answer:
kolezko [41]3 years ago
4 0

Answer:

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.

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3 years ago
Seawater has a ph of 8.1. what is the concentration of oh–?
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PH scale is used to determine how acidic or basic a solution is.
pH can be calculated as follows;
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A balloon contains 11.1 g of nitrogen monoxide gas (NO). how many molecules are in the balloon?
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The number of molecules that are in balloon are = 2.227 x10^23 molecules

<h3> calculation</h3>

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moles is therefore=  11.1 g/30g/mol= 0.37 moles

by use of Avogadro's constant that is

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