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another sample of anhydrous magnesium chloride gave, on electrolysis, 2.24 litre of chlorine at NTP.

Show that these data agree with the law of constant proportions.

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elements no matter from it comes and this is known as the law of constant proportion. So, we have

to prove that the concentration of chlorine is the same from both sources.

- In the given question, we have to prove whether the chlorine is present in the same amount when

different samples were taken.

- As we know that the law of constant proportion states that in the compound, its elements have a

fixed ratio, it does not matter from where they are taken.

- So, it is given that 0.36g of magnesium combines with the chlorine and gives 1.425g of magnesium

chloride.

- The chemical reaction is: \[\text{Mg + C}{{\text{l}}_{2}}\text{ }\to \text{ MgC}{{\text{l}}_{2}}\]

- So, the mass of the chlorine is $\text{1}\text{.425 - 0}\text{.36 = 1}\text{.065g}$.

- Now, if 1.425g of magnesium chloride is produced 1.065g of chlorine then 1g of magnesium

chloride will be produced $\dfrac{1.0625}{1.425}\text{ = 0}\text{.747g}$ of chlorine.

- So, 9.5g of \[\text{MgC}{{\text{l}}_{2}}\] will produce $\dfrac{2.24}{9.5}\text{ = 0}\text{.235L of

C}{{\text{l}}_{2}}$.

- Now, the molecular mass of chlorine is 71g which occupies \[\text{22}\text{.4d}{{\text{m}}^{3}}\] at

NTP conditions.

- So, \[\text{0}\text{.235d}{{\text{m}}^{3}}\] of volume will have $\dfrac{0.235\text{ }\times \text{

70}\text{.9}}{22.4}\text{ = 0}\text{.744g}$ of chlorine.

- Now, as we can see that the value of the chlorine is close to 1.425g and 9.5g of magnesium

chloride.

Therefore, it follows the law of constant proportion.

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