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quester [9]
3 years ago
6

When magnesium chloride reacts with water, 5.85 L HCl(g) is produced.

Chemistry
2 answers:
pochemuha3 years ago
7 0

Answer: (i) 0.261 moles of HCl, (ii) 0.131 moles of MgCl_2 and (iii) 12.5 grams of MgCl_2

Explanation: The balanced equation for the formation of HCl by the reaction magnesium chloride with water is:

MgCl_2+2H_2O\rightarrow 2HCl+Mg(OH)_2

From above balanced equation, there is 1:2 mol ratio between magnesium chloride and HCl.

As per the given information, 5.85 L of HCl gas is produced. here, temperature and pressure is not mentioned, so let's assume STP conditions.

At STP, volume of 1 mol of a gas is 22.4 L. With the help of this, we can calculate the moles of HCl present in 5.85 L.

5.85LHCl(\frac{1mol}{22.4L})

= 0.261 mol HCl

As there is 1:2 mol ratio between magnesium chloride and HCl, we can calculate the moles of magnesium chloride from the above calculated moles of HCl as:

0.261molHCl(\frac{1molMgCl_2}{2molHCl})

= 0.131 mol MgCl_2

Molar mass of magnesium chloride is given as 95.2 gram per mol. On multiplying the moles by molar mass we can calculate its mass reacted.

0.131molMgCl_2(\frac{95.2g}{1mol})

= 12.5 g MgCl_2

amid [387]3 years ago
3 0

Answer: How many moles of HCl was produced?

⇒ 0.261 moles of HCl

How many moles of MgCl2 reacted?

⇒ 0.131 moles of MgCl2

What mass of MgCl2 reacted?

⇒ 12.4 g MgCl2

Explanation:

i just did it

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Answer:

a) 7.0.

b) Nickel sulfate hepta hydrate.

c) 280.83 g/mol.

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<u><em>a) What is the formula of the hydrate?</em></u>

The mass of the hydrated sample (NiSO₄.xH₂O) = 5.0 g,

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∴ no. of moles of anhydrous salt (NiSO₄) = mass/molar mass = (2.755 g)/(154.75 g/mol) = 0.0178 mol.

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<u><em>b) What is the full chemical name for the hydrate?</em></u>

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<u><em>c) What is the molar mass of the hydrate? </em></u>

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<em><u>d) What is the mass % of water in the hydrate?</u></em>

The mass % of water = (mass of water)/(mass of hydrated sample) x 100 = (2.245 g)/(5.0 g) x 100 = 44.9%.

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