Given 25.0 g of Al, how many grams of the product Al2O3 could be produced?
4 Al + 3 O2 = 2 Al2O3
or, Al + (3/4) O2 = (2/4) Al2O3
25 gm Al = (25/27) = 0.93 moles of Al
1 mole Aluminum produces 0.5 mole of Al2O3
0.93 moles of Aluminum produces (0.5 X 0.93) = 0.465 moles of Al2O3
Molar weight of Al2O3 = ( 27X2) + (16 X3) = 102
0.465 moles of Al2O3 = 0.465 X 102 = 47.43 gms of Al2O3
Given 25.0 g of Al, how many grams of the product Al2O3 could be produced?
Given 25.0 g of O2, how many grams of the product Al2O3 could be produced?
Given 25.0 g of O2, how many grams of the product Al2O3 could be produced?
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Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem