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

Answer:

$m_{H_2O_2}=0.317gH_2O_2$

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:

$n_{H_2O_2}^{by\ BaO_2}=1.50gBaO_2*\frac{1molBaO_2}{169.33gBaO_2}*\frac{1molH_2O_2}{1molBaO_2}=0.00886molH_2O_2\\\\ n_{H_2O_2}^{by\ HCl}=0.0272\frac{gHCl}{mL}*25.0mL *\frac{1molHCl}{36.46gHCl}*\frac{1molH_2O_2}{2molHCl}=0.00933molH_2O_2$

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

$m_{H_2O_2}=0.00933molH_2O_2*\frac{34.02gH_2O_2}{1molH_2O_2}\\\\m_{H_2O_2}=0.317gH_2O_2$

Best regards!