+330
how many grams are in 5.0*10^26 molecules of Cl2
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(Greetings Alan, It is diatomic Chlorine, not carbon).
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This question originally had an anonymously appended, incorrect answer to the chemistry question, and a vulgar-worded (probably why it was deleted) opinion stating this is a math site and not a chemistry site. My comments below reflect this.
--------
The chemistry answer by Anonymous is incorrect.
The correct solution and the method for its derivation are below.
His/her opinion of the site is subjective. There are tutors on this site who know chemistry. Any science question, which relates to applied mathematics is reasonable.
To solve this:
Divide the quantity of the molecules by Avogadro constant (currently: 6.022141E23/mol). This constant is the number of atoms or molecules per molar mass of an element or compound.
5.0*10E26 molecules (Cl2)/ 6.022141E23/mol = 830.3 mols of Cl2
Look up the Relative atomic mass (aka Standard atomic weight) of Cl (Chlorine). It is 35.45. Pure Chlorine, in the gas state, usually exists in a diatomic form (Cl2). This condition is indicated by the subscript. Multiply the Relative atomic mass by this subscript value (2): 35.45 *2 = 70.90. (Note that diatomic forms are considered molecules).
The Relative atomic mass of diatomic Chlorine is 70.90. Convert to gram mass (by multiplying by 1g). 70.90 * 1g = 70.90g. This is the gram molecular mass and it equals 1 mol: 70.90g of Cl2 = 1 mol. Restated: for each mol of Cl2 there are 70.90 grams of Cl2.*
Multiply the 830.3 mols of Cl2 by 70.90g/mol = 58873.2g of Cl2. (58.8732Kg of Cl2).
This is slightly less chlorine than required to maintain "chemical pasteurization” of an Olympic-size non-comercial pool.
~~D~~
+33654 Avogadro's number NA = 6.0221415.1023 molecules per mole
One mole of C12 is 12 grams.
This means 6.0221415.1023 molecules of C12 is 12 grams.
So 5*1026 molecules of C12 is (12*5*1026)/(6.0221415*1023) grams
(12×5×1026)(6.0221415×1023)=9963.2331787620732592 grams
But see David's reply below.
+330
how many grams are in 5.0*10^26 molecules of Cl2
---------
(Greetings Alan, It is diatomic Chlorine, not carbon).
----
This question originally had an anonymously appended, incorrect answer to the chemistry question, and a vulgar-worded (probably why it was deleted) opinion stating this is a math site and not a chemistry site. My comments below reflect this.
--------
The chemistry answer by Anonymous is incorrect.
The correct solution and the method for its derivation are below.
His/her opinion of the site is subjective. There are tutors on this site who know chemistry. Any science question, which relates to applied mathematics is reasonable.
To solve this:
Divide the quantity of the molecules by Avogadro constant (currently: 6.022141E23/mol). This constant is the number of atoms or molecules per molar mass of an element or compound.
5.0*10E26 molecules (Cl2)/ 6.022141E23/mol = 830.3 mols of Cl2
Look up the Relative atomic mass (aka Standard atomic weight) of Cl (Chlorine). It is 35.45. Pure Chlorine, in the gas state, usually exists in a diatomic form (Cl2). This condition is indicated by the subscript. Multiply the Relative atomic mass by this subscript value (2): 35.45 *2 = 70.90. (Note that diatomic forms are considered molecules).
The Relative atomic mass of diatomic Chlorine is 70.90. Convert to gram mass (by multiplying by 1g). 70.90 * 1g = 70.90g. This is the gram molecular mass and it equals 1 mol: 70.90g of Cl2 = 1 mol. Restated: for each mol of Cl2 there are 70.90 grams of Cl2.*
Multiply the 830.3 mols of Cl2 by 70.90g/mol = 58873.2g of Cl2. (58.8732Kg of Cl2).
This is slightly less chlorine than required to maintain "chemical pasteurization” of an Olympic-size non-comercial pool.
~~D~~
