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love history [14]
3 years ago
7

What mass of aluminum is produced by the decomposition of 5.0 kg al2o3?

Chemistry
2 answers:
Nina [5.8K]3 years ago
7 0
The  mass for  of aluminum that is produced  by  the decomposition  of  5.0 Kg Al2O3 is 2647 g or 2.647  Kg

          calculation
  Write  the equation for decomposition  of Al2O3

Al2O3 = 2Al  + 3 O2

find the  moles  of  Al2O3 =  mass/molar mass

convert  5 Kg  to g   = 5 x1000 = 5000 grams
molar mass of  Al2O3 =  27 x2 + 16 x3  = 102 g/mol

 moles =5000 g/  102 g/mol = 49.0196 moles

by use  of mole ratio between Al2O3 to  Al  which is 1:2  the moles of Al = 49.0196 x2 =98.0392  moles


mass of  Al = moles x molar  mass

= 98.0392 moles x  27g/mol = 2647  grams  or 2647/1000 = 2.647 Kg


solong [7]3 years ago
3 0
<span>Answer: 2.7 kg


Explanation:


1) Find the molar mass of Al₂O₃, using the atomic masses of Al and O:
</span>

<span>2x27.0g/mol + 3x16.0g/mol = 102.0 g/mol


2) Find the ratio of Al to </span><span>Al₂O₃:
</span>

<span>2x27.0 / 102.0 = 54.0/102.0 = 27.0/51.0 = 9.0/17.0


3) Use proportionality:

</span>9.0 Kg Al / 17.0 kg <span>Al₂O₃ = x / 5.0 kg
</span>

<span>⇒ x = 5.0kg </span><span>Al₂O₃ x (9.0 kg Al/ 17.0 Kg) </span><span>Al₂O₃</span><span />

<span>x = 2.65 kg = 2.7 Kg
</span><span>
</span><span>
</span><span>Al = 2.7 kg Al</span>

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erik [133]

Correct Question:

A chemist measures the enthalpy change ΔH during the following reaction: Fe(s) + 2HCl(g)-->FeCl2(s) + H2 ΔH=-157.0 kJ. Use this information to complete the table below. Round each of your answers to the nearest kJ/mol

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Explanation:

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Hello,

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