Question

If 2.45 g of iron are placed in 1,5 L of 0.25M HCl, how many grams of FeCl2 are obtained? Identify the limiting and excess reactants in this single replacement reaction. Fe + 2HCl = FeCl2 + H2

Answer 1

`m_(FeCl_2)=0.652gFeCl_2`

Step-by-step explanation:

Hello there!

In this case, according to the given information and the chemical reaction, whereby iron and hydrochloric acid react in a 1:2 mole ratio, it is firstly necessary to calculate the moles of iron (II) chloride from each reactant in order to figure out the limiting reactant:

`n_(FeCl_2)=2.45gFe*(1molFe)/(55.845gFe)*(1molFeCl_2)/(1molFe)=0.0439molFeCl_2\\\\ n_(FeCl_2)=1.5L*0.25(molHCl)/(L) *(1molHCl)/(36.46gHCl)*(1molFeCl_2)/(2molHCl)=0.00514molFeCl_2`

In such a way, we infer the maximum moles of FeCl2 product are yielded by HCl, for which it is the limiting reactant. Finally, we calculate the grams of product by using its molar mass as shown below:

`m_(FeCl_2)=0.00514molFeCl_2*(126.75gFeCl_2)/(1molFeCl_2) \\\\m_(FeCl_2)=0.652gFeCl_2`

Regards!