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irga5000 [103]
3 years ago
7

Two samples of carbon tetrachloride were decomposed into their constituent elements. One sample produced 38.9 g of carbon and 45

1 g of chlorine, and the other sample produced 14.8 g of carbon and 135 g of chlorine. Are these results consistent with the law of definite proportions? Show why or why not.
Chemistry
1 answer:
Nataliya [291]3 years ago
3 0

Answer:

No.

Explanation:

The results mentioned are <u>not consistent </u>with the law of definite proportions.

Law of definite proportions states that a chemical compound contains exactly the same elements in the same proportion by weight independent of its source and method of it's preparation.

In the given question, the first sample contains 38.9 g of carbon and 451 g of chlorine that means the sample has 8% of carbon and 92% of chlorine.

On the other hand, second sample contains 14.8 g of carbon and 135 g of chlorine which means that this sample has 10% of carbon and 90% of chlorine.

Since the constituent elements in both the samples are not in fixed and constant proportions (by mass), the law of definite proportions fails here.

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Entropy change is defined only along the path of an internally reversible process path.

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Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms in
avanturin [10]
<span>5.5×10−2M in calcium chloride and 8.0×10−2M in magnesium nitrate.
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Calcium chloride = CaCl2

Ionization equation: CaCl2 ---> Ca (2+) + 2 Cl (-)

=> Molar ratios: 1 mol of CaCl2 : 1 mol Ca(2+) : 2 mol Cl(-)

Calculate the number of moles of CaCl2 in 1.5 liters of 5.5 * 10^-2 M solution

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=> 0.0825 mol Ca(2+)

2) Number of phosphate ions needed to react with 0.0825 mol Ca(2+)

formula of phospahte ion: PO4 (3-)

molar ratio: 2PO4(3-) + 3Ca(2+) = Ca3 (PO4)2

Proportion: 2 mol PO4(3-) / 3 mol Ca(2+) = x / 0.0825 mol Ca(2+)

=> x = 0.0825 coml Ca(2+) * 2 mol PO4(3-) / 3 mol Ca(2+) = 0.055 mol PO4(3-)

3) Content of Mg(2+) ions

Ionization equation: Mg (NO3)2 ----> Mg(2+) + 2 NO3 (-)

Molar ratios: 1 mol Mg(NO3)2 : 1 mol Mg(2+) + 2 mol NO3(-)

number of moles of Mg(NO3)2 in 1.5 liter of 8.0 * 10^-2 M solution

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ions of Mg(2+) = 0.12 mol Mg(NO3)2 * 1 mol Mg(2+) / mol Mg(NO3)2 = 0.12 mol Mg(2+)

4) Number of phosphate ions needed to react with 0.12 mol Mg(2+)

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=> mass in grams = 0.215 mol * 164 g/mol = 35.26 g

Answer: 35.26 g of sodium phosphate
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