Question

If 25.0g solid iron (III) sulfide reacts with 25.0g gaseous hydrogen chloride to form solid iron (III) chloride

and 5.61g hydrogen sulfide gas, what is the percent yield of the reaction?

(Please show work)

Answer 1

`Y=48\%`

Step-by-step explanation:

Hello!

In this case, since the described chemical reaction is:

`Fe_2S_3+6HCl\rightarrow 3H_2S+2FeCl_3`

We can see the 6:2 mole ratio between hydrogen chloride (molar mass = 36.46 g/mol) and hydrogen sulfide (molar mass = 34.09 g/mol) and 1:3 between iron (III) sulfide (molar mass = 207.91 g/mol) and hydrogen sulfide. In such a way, we can compute the yielded moles of hydrogen sulfide by each reactant in order to identify the limiting one:

`n_(H_2S)^(by HCl)=25.0gHCl*(1molHCl)/(36.46gHCl)*(3molH_2S)/(6molHCl) =0.343molH_2S\\\\n_(H_2S)^(by Fe_2S_3)=25.0gFe_2S_3*(1molFe_2S_3)/(207.91gFe_2S_3)*(3molH_2S)/(1molFe_2S_3) =0.361molH_2S`

It means that the HCl is the liming reactant as it produces less moles of hydrogen chloride than the iron (III) sulfide. Therefore, the theoretical yield in grams is:

`m_(H_2S) =0.343molH_2S_2S*(1molH_2S)/(34.09gH_2S)\\\\m_(H_2S)=11.7g`

Thus, the percent yield is:

`Y=(5.61g)/(11.7g)*100\%\\\\Y=48\%`

Best regards!