Question

For the following reaction, 5.22 grams of aluminum oxide are mixed with excess sulfuric acid. The reaction yields 12.9 grams of aluminum sulfate. aluminum oxide (s) + sulfuric acid (aq) aluminum sulfate (aq) + water (l) What is the theoretical yield of aluminum sulfate ?

Answer 1

`m_(Al_2(SO_4)_3)=17.5gAl_2(SO_4)_3`

Step-by-step explanation:

Hello,

In this case, the undergoing balanced chemical reaction is:

`Al_2O_3(s)+3H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+3H_2O(l)`

Thus, as 5.22 grams of aluminium oxide reacts, the required yielded amount of aluminium sulfate results:

`m_(Al_2(SO_4)_3)=5.22gAl_2O_3*(1molAl_2O_3)/(102gAl_2O_3)*(1molAl_2(SO_4)_3)/(1molAl_2O_3)*(342gAl_2(SO_4)_3)/(1molAl_2(SO_4)_3) \\\\m_(Al_2(SO_4)_3)=17.5gAl_2(SO_4)_3`

Moreover, the percent yield is:

`Y=(12.9g)/(17.5g) *100\%=73.7\%`

Best regards.