Question

common salt was obtained from two different sources in one sample chlorine was 60.75% and in another sample 3.888g chlorine was present in 6.4g of common salt . illustrate the law of conservation of mass

Answer 1

Note: Common Salt = Sodium Chloride = NaCl

According to Law of Constant Proportion, Mass of an element (or its mass percentage) in a particular compound is always constant, no matter how it is prepared.

So, by law of constant proportion, mass of chlorine will be constant in every Molecule of the compound NaCl.

Now, Let's verify it.

1.)
Atomic Mass of Chlorine = 35.5g
Atomic Mass of Sodium = 23g
Molar Mass of NaCl = 58.5g

Percentage of Chlorine in NaCl:

=(Mass of Chlorine)×100/(Total Mass of molecule)
=(35.5 ×100)/58 = 61.20% -------- (1)

which is approximately equal to 60.75%, which is the given calculated quantity of Chlorine in the given Common Salt .

By this, The Law of Constant Proportion is justified.

2.)
Atomic Mass of Chlorine = 35.5g
Atomic Mass of Sodium = 23g
Molar Mass of NaCl = 58.5g

Mass Percentage of Chlorine in NaCl = 61.20%
(from Eq 1)

Now, the mass of Chlorine present in 6.4g NaCl is:

= [(Mass Percentage of Chlorine)/100] × 6.4
= (61.20/100)×6.4
= 3.9g

which is approximately equal to 3.888g, the given calculated quantity of Chlorine in common salt.
By this, Law of Constant Proportion is justified.

Hope this helps :)

Answer 2

Answer:

above answer is ridiculous