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

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

2.7 kg

Explanation:

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


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

2) Find the ratio of Al to Al₂O₃:


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

3) Use proportionality:

9.0 Kg Al / 17.0 kg Al₂O₃ = x / 5.0 kg


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

x = 2.65 kg = 2.7 Kg


Al = 2.7 kg Al

the catch is that the top numbers are atomic masses the bottom numbers are the numbers of protons and electrons in an uncharged atom. they are the number of that atoms as you would find them on the periodic table. further, the numbers on the left are used to determine the missing numbers on the right

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

The answer is celsius