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natulia [17]
3 years ago
14

A sample weighing 3.110 g is a mixture of Fe 2 O 3 (molar mass = 159.69 g/mol) and Al 2 O 3 (molar mass = 101.96 g/mol). When he

at and a stream of H 2 gas is applied to the sample, the Fe 2 O 3 reacts to form metallic Fe and H 2 O ( g ) . The Al 2 O 3 does not react. If the sample residue (the solid species remaining after the reaction) weighs 2.387 g, what is the mass fraction of Fe 2 O 3 in the original sample?
Chemistry
1 answer:
grandymaker [24]3 years ago
5 0

Answer:

The mass fraction of ferric oxide in the original sample :\frac{723}{3110}

Explanation:

Mass of the mixture = 3.110 g

Mass of Fe_2O_3=x

Mass of Al_2O_3=y

After heating the mixture it allowed to react with hydrogen gas in which all the ferric oxide reacted to form metallic iron and water vapors where as aluminum oxide did not react.

Fe_2O_3(s)+3H_2(g)\rightarrow 2Fe(s)+3H_2O(g)

Mass of mixture left after all the ferric oxide has reacted = 2.387 g

Mass of mixture left after all the ferric oxide has reacted = y

x=3.110 g- y=3.110 g - 2.387 g = 0.723 g

The mass fraction of ferric oxide in the original sample :

\frac{0.723 g}{3.110 g}=\frac{723}{3110}

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arsen [322]

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hope this helps! :)

6 0
3 years ago
4. Al2O3 (s) + 6HCl (aq) → 2AlCl3 (aq) + 3H20(1) Find the mass of AlCl3 that is produced when 10.0 grams of Al2O3 react with 10.
slava [35]

Answer:

Are produced 12,1 g of AlCl₃ and 5,33 g of Al₂O₃ are left over

Explanation:

For the reaction:

Al₂O₃ (s) + 6 HCl (aq) → 2AlCl₃ (aq) + 3H₂0(l)

10,0g of Al₂O₃ are:

10,0g ₓ\frac{1mol}{102g} = <em>0,0980 moles</em>

And 10,0g of HCl are:

10,0 gₓ\frac{1mol}{36,5g} = <em>0,274 moles</em>

<em />

For a total reaction of 0,274 moles of HCl you need:

0,274×\frac{1molesAl_{2}O_3}{6 mole HCl} = <em>0,0457 moles of Al₂O₃</em>

Thus, limiting reactant is HCl

The grams produced of AlCl₃ are:

0,274 moles HCl ×\frac{2 moles AlCl_{3}}{6 moles HCl} × 133\frac{g}{mol} = <em>12,1 g of AlCl₃</em>

<em />

The moles of Al₂O₃ that don't react are:

0,0980 moles - 0,0457 moles =<em> </em>0,0523 moles

And its mass is:

0,0523 molesₓ\frac{102g}{1mol} = <em>5,33 g of Al₂O₃ </em>

<em />

I hope it helps!

7 0
3 years ago
Calculate the ph of a 0.40 m solution of sodium benzoate (nac6h5coo) given that the ka of benzoic acid (c6h5cooh) is 6.50 x 10-5
asambeis [7]
Hello!

The dissociation reaction for Benzoic Acid is the following:

C₆H₅COOH + H₂O ⇄ C₆H₅COO⁻ + H₃O⁺

The Ka expression is the following and we clear for the concentration of H₃O⁺(X) assuming that the dissociation is little so we can rule it out in the denominator of the equation:

Ka= \frac{[C_6H_5COO^{-}]*[H_3O^{+}] }{[C_6H_5COOH]}=\frac{X*X }{0,40 -X}  (assume: 0,40-X\approx0,40)\\  \\ X= \sqrt{0,40*6,50*10^{-5} }=0.00510M \\  \\ pH=-log([H_3O^{+}]=2,29

So, the pH of this Benzoic Acid solution is 2,29

Have a nice day!


3 0
3 years ago
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lord [1]
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8 0
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