Why is CCl4 classified as a non polar molecule?
1 answer:
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Answer:
Explanation:
To solve this problem, we must understand the relationship between mass of a substance and the number of atoms.
Atoms are the smallest indivisible particles of any matter. A substance can be made up of several number of atoms in their space.
The mass of any substance is a function of the amount of atoms its contains.
The mass of a substance is related in chemistry to the amount of atoms its contains using the parameter called the number of moles.
A mole is the amount of substance that contains the Avogadro's number of particles. This number is 6.02 x 10²³ particles. The particles here can be protons, neutrons, electrons, atoms e.t.c.
Now,
Number of moles =
Molar mass of copper = 63.6g/mole
Number of moles = = 0.03mole
Since 1 mole of a substance contains 6.02 x 10²³atoms
0.03 mole of copper will contain 0.03 x 6.02 x 10²³atoms
= 1.89 x 10²² atoms
He needs to add 1.89 x 10²² atoms to make 2g of the sample.
Answer:
a) Percentage by mass of carbon: 18.3%
Percentage by mass of hydrogen: 0.77%
b) Percentage by mass of chlorine: 80.37%
c) Molecular formula:
Explanation:
Firstly, the mass of carbon must be determined by using a conversion factor:
The same process is used to calculate the amount of hydrogen:
The percentage by mass of carbon and hydrogen are calculated as follows:
%C= 18.3%
%H=0.77%
From the precipation data it is possible obtain the amount of chlorine present in the compound:
= 0.43g AgCl
Let's calculate the percentage by mass of chlorine:
%Cl== 80.37%
Assuming that we have 100g of the compound, it is possible to determine the number of moles of each element in the compound:
Dividing each of the quantities above by the smallest (0.77mol), the subscripts in a tentative formula would be
≈ 2
≈3
The empirical formula for the compound is:
The mass of this empirical formula is:
mass of C + mass of H + mass of Cl= 24g +1+ 106.35 =131.35g
This mass matches with the molar mass, which means that the supscript in the molecular formula are the same of the empirical one.