How many grams of aluminum oxide would form if 15.2 moles of aluminum burned

Your answer would be 637.25g

6.25 moles Al2O3 Since all provided numbers are moles, there is no need for conversion. Rather, use a molar ratio: 12.5 Multiply across the top, 12.5 x 2, which gives you 25, before dividing that by the denominator (4). This gives you the final answer of 6.25 moles of Al2O3. Hope this helps!

When 350 kJ are released there are formed 41,98 g of aluminium oxide. Explanation: For the reaction: 2Al (s) + Fe₂O₃ (s) → 2Fe (s) + Al₂O₃(s) There are produced 850 kJ. 350 kJ of energy produced are when are formed: 350 kJ × = 0,412 moles of Aluminium oxide. As molar mass of aluminium oxide is 101,96 g/mol. The grams in 0,412 moles of Al₂O₃ are: 0,412 moles Al_{2}O_{3} × = 41,98 g Thus, when 350 kJ are released there are formed 41,98 g of aluminium oxide. I hope it helps!

1mole  =  850Kjwhat  about  350kj=1mole  x350/850  =  0.412  moles mass  of  Al =   moles  of  Al x  molar  mass of  Al =  0.412mol  x  27  g/mol  =  11.124  grams

Also Read :   Draw both the organic and inorganic intermediate species. include nonbonding electrons and charges, where applicable. include hydrogen

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