Question

What amount of hydrogen peroxide should result ( theoretical yield) when 1.50g of barium peroxide is treated with 25.0 mL of hydrochloric acid solution containing 0.0272 g of HCl per mL

Answer 1

`m_(H_2O_2)=0.317gH_2O_2`

Step-by-step explanation:

Hello!

In this case, for the chemical reaction between hydrochloric acid and barium peroxide is:

`BaO_2(s)+2HCl(aq)\rightarrow H_2O_2(aq)+BaCl_2(aq)`

Thus, since the barium peroxide (169.33 g/mol) and hydrochloric acid (36.45 g/mol) are reacting in a 1:2 mole ratio, we need to identify the limiting reactant first by computing the yielded moles of hydrogen peroxide by each reactant:

`n_(H_2O_2)^(by\ BaO_2)=1.50gBaO_2*(1molBaO_2)/(169.33gBaO_2)*(1molH_2O_2)/(1molBaO_2)=0.00886molH_2O_2\\\\ n_(H_2O_2)^(by\ HCl)=0.0272(gHCl)/(mL)*25.0mL *(1molHCl)/(36.46gHCl)*(1molH_2O_2)/(2molHCl)=0.00933molH_2O_2`

That's why the HCl is the limiting reactant, so the resulting mass of hydrogen peroxide, theoretical yield, is:

`m_(H_2O_2)=0.00933molH_2O_2*(34.02gH_2O_2)/(1molH_2O_2)\\\\m_(H_2O_2)=0.317gH_2O_2`

Best regards!