Been getting the wrong answer for so many times I\'ve tried. ± Core Chemistry Sk

Question

Been getting the wrong answer for so many times I've tried.

± Core Chemistry Skill: Calculating Moles of Product from a Limiting Reactant Part A What is the theoretical yield of aluminum oxide if 1.80 mol of aluminum metal is exposed to 1.65 mol of oxygen? When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2 03, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: Express your answer with the appropriate units. Hints alueUnits Submit My Answers Give Up

Explanation / Answer

we have the Balanced chemical equation as:

4 Al + 3 O2 ---> 2 Al2O3

4 mol of Al reacts with 3 mol of O2

for 1.8 mol of Al, 1.35 mol of O2 is required

But we have 1.65 mol of O2

so, Al is limiting reagent

we will use Al in further calculation

Molar mass of Al2O3 = 2*MM(Al) + 3*MM(O)

= 2*26.98 + 3*16.0

= 101.96 g/mol

From balanced chemical reaction, we see that

when 4 mol of Al reacts, 2 mol of Al2O3 is formed

mol of Al2O3 formed = (2/4)* moles of Al

= (2/4)*1.8

= 0.9 mol

we have below equation to be used:

mass of Al2O3 = number of mol * molar mass

= 0.9*1.02*10^2

= 91.8 g

Answer: = 91.8 g

Feel free to comment below if you have any doubts or if this answer do not work. I will correct it and submit again if you let me know

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