+0  
 
+1
49
3
avatar+1397 

Help Me Please

 

Solve the problem.

Express the answer using proper significant figures and units. Refer to the periodic table as needed.

 

Consider the reaction 2 Al(s) + Fe2O3(s) → 2 Fe(I) + Al2O3(s). If 60.0 g of Al is reacted with excess Fe2O3, determine the amount (in moles) and mass (in grams) of Al2O3 produced. (MAl2O3= 101.96 g/mol)

Separate your answers with a semicolon.

 Dec 27, 2018
edited by ManuelBautista2019  Dec 28, 2018
 #1
avatar+15350 
+4

Al atomic mass  26.98 gm/mole

 

60.0 / 26.98 = 2.22 moles of Aluminum (3 sig digits)

 

each 2 moles of Aluminum produce ONE mole of Aluminum oxide

 

2.22 moles Al / 2 moles Al/ Al2O3   = 1.11 moles Aluminum oxide

1.11 moles Aluminum Oxide   *   101.96 g/mole = 113 gm aluminum oxide (3 sig digits)

 Dec 28, 2018
 #2
avatar+1397 
+2

what does ''sig digits'' stands for?

 Dec 28, 2018
 #3
avatar+95171 
+2

sig digits = significant digits.

Melody  Dec 28, 2018

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