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#11.) When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 77.4 mol of iron in the rusting reaction?

4Fe(s) + 3O2(g) → 2Fe2O3(s)

Select one:
a. 58
b. 100
c. 77
d. 120

#13.) For the reaction CH4 + 2O2 → CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 161.0 g of methane?

Select one:
a. 10.03
b. 20.06
c. 2584
d. 3.351

Respuesta :

PBCHEM

Answer 1) Option A) 58.05


In the given reaction of iron forming rust when reacts with the oxygen.


[tex] 4 Fe_{(s)} + 3O_{2}_{(g} ----> 2Fe_{2}O_{3}_{(s)} [/tex]


We can clearly see that, 4 moles of iron reacts with 3 moles of oxygen to give 2 moles of iron oxide.


So 4 Fe : 3 O and 77.4 moles of Fe : x moles of O


(3 X 77.4) / 4 = 58.05


So when we solve we get x as 58.05.


Hence the no. of moles of oxygen will be 58.


Answer 2) Option A) 10.03


The number of moles of carbon dioxide produced when 161.0 g of methane undergoes combustion will be 10.03


as we know the molar mass of methane is 16.043 g


As we can see in the reaction the mole ratio is 1:1;


1 mole of methane produces 1 mole of carbondioxide.


So, 161 g / 16.043 g = 10.03 moles of Carbon dioxide.

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