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How to solve the problems of avogadro constant????
Here is one problem of mine:
Calculate the total number of atoms in 8.5g of CH2Cl2. Molar mass of CH2Cl2 is 85 g/mol
Avogadro constant 6.0*10^23
Here is one problem of mine:
Calculate the total number of atoms in 8.5g of CH2Cl2. Molar mass of CH2Cl2 is 85 g/mol
Avogadro constant 6.0*10^23
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#2
the equation for avogadro's constant is
so you can calculate the number of moles coz you've got the mass (8.5g) and you've got the molar mass (85g/mol)
then just sub it into the equation and you're good
so you can calculate the number of moles coz you've got the mass (8.5g) and you've got the molar mass (85g/mol)
then just sub it into the equation and you're good
Spoiler:
I think the answer is
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I think the answer is
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Thx,
So you wanted to say that we need to multiply moles with avogadro constant which is equal to number of molecules divided by atoms.
So you wanted to say that we need to multiply moles with avogadro constant which is equal to number of molecules divided by atoms.
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#4
(Original post by madmahin)
Thx,
So you wanted to say that we need to multiply moles with avogadro constant which is equal to number of molecules divided by atoms.
Thx,
So you wanted to say that we need to multiply moles with avogadro constant which is equal to number of molecules divided by atoms.
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#6
you have to go through a step first using the
mass = Mr x moles
equation first. you have the mass (8.5g) and you have the Mr/molar mass (85) so in order to find the number of moles, you'll have to divide the mass by the Mr.
then you multiply by Avogadro's constant to find the number of molecules or atoms.
mass = Mr x moles
equation first. you have the mass (8.5g) and you have the Mr/molar mass (85) so in order to find the number of moles, you'll have to divide the mass by the Mr.
then you multiply by Avogadro's constant to find the number of molecules or atoms.
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#7
So Avogadro's constant is the number of atoms or molecules in 1 mole of substance. If you have 2 moles of substance, the number of atoms you have would be double Avogadro's constant --> #moles * Avogadro's constant = # of atoms or # of molecules
First you gotta determine the number of moles you have of CH2Cl2: so (8.5g)/(85g/mol) = 0.1mol
Then multiply your answer by Avogadro's constant: 0.1 * 6.022*10^23 = 6.022*10^22 molecules in 8.5g of CH2Cl2
Hope that helps
First you gotta determine the number of moles you have of CH2Cl2: so (8.5g)/(85g/mol) = 0.1mol
Then multiply your answer by Avogadro's constant: 0.1 * 6.022*10^23 = 6.022*10^22 molecules in 8.5g of CH2Cl2
Hope that helps
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#8
(Original post by lordmasterlu)
= 6.022*10^22 molecules in 8.5g of CH2Cl2
= 6.022*10^22 molecules in 8.5g of CH2Cl2
There are 5 atoms (1xC, 2xH & 2xCl) in each molecule of CH2Cl2, hence there will be 5 x 6.02x1023.
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#9
(Original post by Pigster)
The OP asked about the number of atoms in 8.5 g, NOT the number of molecules.
There are 5 atoms (1xC, 2xH & 2xCl) in each molecule of CH2Cl2, hence there will be 5 x 6.02x1023.
The OP asked about the number of atoms in 8.5 g, NOT the number of molecules.
There are 5 atoms (1xC, 2xH & 2xCl) in each molecule of CH2Cl2, hence there will be 5 x 6.02x1023.
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#10
(Original post by nyxnko_)
the equation for avogadro's constant is
so you can calculate the number of moles coz you've got the mass (8.5g) and you've got the molar mass (85g/mol)
then just sub it into the equation and you're good
the equation for avogadro's constant is
so you can calculate the number of moles coz you've got the mass (8.5g) and you've got the molar mass (85g/mol)
then just sub it into the equation and you're good
Spoiler:
I think the answer is
Show
I think the answer is
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#12
(Original post by nyxnko_)
sorry? it's really bad, isn't it?
sorry? it's really bad, isn't it?
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#13
(Original post by alow)
In general when you're writing text in LaTeX it should be upright, this means on TSR you have to use \text{...}. Also to do a displayed fraction, use \dfrac{numerator}{denominator}.
In general when you're writing text in LaTeX it should be upright, this means on TSR you have to use \text{...}. Also to do a displayed fraction, use \dfrac{numerator}{denominator}.
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