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docker41 [41]
3 years ago
5

A 1.167 grams sample of hydrated Nickel (II) Chloride is heated until a constant mass is achieved. The constant mass of the samp

le is .750 grams. What is the formula and name of the hydrate?
Chemistry
1 answer:
svetoff [14.1K]3 years ago
6 0

Answer:

NiCl₂·4H₂O, its name being nickel (II) chloride tetrahydrate.

Explanation:

The constant mass achieved after heating is the mass of anhydrous nickel (II) chloride, NiCl₂. While the mass lost was water.

  • Mass lost = 1.167 g - 0.750 g = 0.417 g

Now we <u>convert 0.750 g of NiCl₂ into moles</u>, using <em>its molar mass</em>:

  • 0.750 g NiCl₂ ÷ 129.6 g/mol = 0.0058 mol NiCl₂

Then we <u>convert 0.417 g of H₂O into moles</u>:

  • 0.417 g H₂O ÷ 18 g/mol = 0.0231 mol H₂O

With the above information we can calculate that the number of H₂O moles is 4 times higher than the number of NiCl₂ moles.

Meaning that <em>the formula of the hydrate is NiCl₂·4H₂O</em>, its name being nickel (II) chloride tetrahydrate.

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Explanation:

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This is the conclusion of equations and evidences that prove that the universe has been and continuous to expand: since it has been expanding, there was a moment when it was as small and dense as it is possible.

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3 years ago
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Answer:

K(48.5°C) = 1.017 E-8 s-1

Explanation:

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at T1 = 25°C (298 K) ⇒ K1 = 3.32 E-10 s-1

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Arrhenius eq:

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⇒ Ln K1 = Ln(A) - [Ea/R)*(1/T1)]..........(1)

⇒ Ln K2 = Ln(A) - [(Ea/R)*(1/T2)].............(2)

(1)/(2):

⇒ Ln (K1/K2) = (Ea/R)* (1/T2-1/T1)

⇒ Ln (K1/K2) = (116 KJ/mol/8.3134 E-3 KJ/K.mol)*(1/321.5 K - 1/298 K)

⇒ Ln (K1/K2) = (13952.37 K)*(- 2.453 E-4 K-1)

⇒ Ln (K1/K2) = - 3.422

⇒ K1/K2 = e∧(-3.422)

⇒ (3.32 E-10 s-1)/K2 = 0.0326

⇒ K2 = (3.32 E-10 s-1)/0.0326

⇒ K2 = 1.017 E-8 s-1

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