Question

Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. how many grams of aluminum sulfate would be formed if 250 g hso completely reacted with aluminum?

Answer 1

atomic weights S-32 O-16 Al-27 H-1
aluminium sulfate 250g= 2.55 mol (250/98)
3Al + 2H2SO4 ---------> Al2(SO4)3 + 2H2
therefore two parts of sulfuric acid produces one part of aluminum sulfate.

2.55mol /2 =1.275 mol 1.275mols of aluminium sulfate is produced.

1.275mol s multiplied by aluminium sulfate's molar mass (342g/mol) gives it's mass in grams..

how many grams of aluminium sulfate produced ? 436.22 g HOPE THIS HELPS GOOD LUCK

Answer 2

`m_(Al_2(SO_4)_3)=291gAl_2(SO_4)_3`

Step-by-step explanation:

Hello,

In this case, the undergoing reaction is:

`2Al(s)+3H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+3H_2(g)`

In such a way, from the 250 g of sulfuric acid that completely reacts with the aliminium, the yielded grams of aluminium sulfate are computed by considering the 3 to 1 molar relationship between sulfuric acid and aluminium sulfate and the corresponding molar masses of 98 g/mol and 342 g/mol respectively:

`m_(Al_2(SO_4)_3)=250gH_2SO_4*(1molH_2SO_4)/(98gH_2SO_4)*(1molAl_2(SO_4)_3)/(3molH_2SO_4) *(342gAl_2(SO_4)_3)/(1molAl_2(SO_4)_3) \\\\m_(Al_2(SO_4)_3)=291gAl_2(SO_4)_3`

Best regards.