Question

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Answer 1

* Limiting reagent: potassium.

*
`m_(Cl_2)^(excess)=2.47gCl_2`

Step-by-step explanation:

Hello,

In this case, the undergoing chemical reaction is:

`2K(s)+Cl_2(g)\rightarrow 2KCl`

In such a way, the reacting moles of chlorine are:

`n_(Cl_2)=7.00g*(1molCl_2)/(70.9gCl_2)=0.0987molCl_2`

Now, the amount of chlorine gas that would react with 5.00 g of potassium result:

`n_(Cl_2)^(consumed)=5.00g*(1molK)/(39.1gK)*(1molCl_2)/(2molK)=0.0639molCl_2`

Thus, the chlorine will be in excess and the potassium will be the limiting reagent. Therefore, the mass of excess chlorine turns out:

`m_(Cl_2)^(excess)=(0.0987-0.0639)molCl_2*(70.9gCl_2)/(1molCl_2)=2.47gCl_2`

Best regards.