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Nostrana [21]
3 years ago
15

When the reddish-brown mercury(ii) oxide (hgo) is heated, it decomposes to its elements, liquid mercury metal and oxygen gas. if

1.19 g hgo is decomposed to hg, calculate the mass of the pure hg metal produced. 2 hgo(s) 2 hg(l) + o2(g)?
Chemistry
1 answer:
konstantin123 [22]3 years ago
7 0
2HgO----->  2Hg  +  O2

find  the  moles  of  HgO,

moles=mass/molar  mass

1.19g/216.59(molar  mass  of  HgO) =   5.49  x10^-3moles

by  use   of  mole  ratio  between  HgO  and Hg  which  is  2:2    or  1:1  the moles   of  Hg  is  also   5.49  x10^-3  moles

mass  of  Hg  is  therefore  =  (5.49  x10^-3)  x  200.59  =  1.101  grams
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Answer:

0.7g of HCl

Explanation:

First, let us write a balanced equation for the reaction between HCl and Al(OH)3.

This is illustrated below:

Al(OH)3 + 3HCl —> AlCl3 + 3H2O

Next, let us obtain the masses of Al(OH)3 and HCl that reacted together according to the equation. This can be achieved as shown below:

Molar Mass of Al(OH)3 = 27 + 3(16+1)

= 27 + 3(17) = 27 + 51 = 78g/mol.

Molar Mass of HCl = 1 + 35.5 = 36.5g/mol

Mass of HCl from the balanced equation = 3 x 36.5 = 109.5g

Now we can obtain the mass of HCl that would react with 0.5g of Al(OH)3. This can be achieved as follow:

Al(OH)3 + 3HCl —> AlCl3 + 3H2O

From the equation above,

78g of Al(OH)3 reacted with 109.5g of HCl.

Therefore, 0.5g of Al(OH)3 will react with = (0.5 x 109.5)/78 = 0.7g of HCl

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3 years ago
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