The corrosion of aluminum in cookware is prevented as the aluminum metal reacts with oxygen gas in the air producing a protective coat of aluminum oxide. Aluminum) Al+3 (Oxygen) O-2

Al + O2 > Product(?
a) Write the balanced equation for the reaction.

b) How many grams of oxygen gas is used in the reaction if 3.25 moles of aluminum oxide is produced?

c) How many grams of aluminum oxide will be produced by the reaction

d) If the reaction gave an actual yield of 228.4 g, what is the percent yield for the reaction?

Explanation:

 2Al    +    3 O₂   =    Al₂O₃

2 moles    3 moles        1 mole

b )

1 mole of aluminium oxide is produced from 3 moles of oxygen gas

3.25 moles of aluminium oxide is produced from 3 x 3.25 moles of oxygen

= 9.75 moles of oxygen

= 9.75 x 32grams of oxygen

= 312 grams of oxygen.

c )

3.25 moles of aluminium oxide = 3.25 x 102 = 331.5 grams of aluminium oxide

( molecular weight of aluminium oxide = 102 )

d ) actual yield = 228.4 gram

percent yield = 228.4 x 100 / 331.5

= 69 % approx .

passing a magnet thought the

mixture , because iron gets attracted to magnet .

c. 75.7

i think that is the right