Considering the reaction stoichiometry, you obtain:
The balanced reaction is:
Pb²⁺(aq) + 2 KCl(aq) → PbCl₂(s) + 2 K⁺(aq)
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
The molar mass of each compound or ion is:
Then, by reaction stoichiometry, the following amount of mass of each compound participate in the reaction:
A sample of water was found to contain 2.6x10⁻³ mole Pb²⁺.
a) Then you can apply the following rule of three: if by stoichiometry 2 moles of Pb²⁺ react with 149.1 grams of KCl, 2.6x10⁻³ moles of Pb²⁺ react with how much mass of KCl?
[tex]mass of KCl=\frac{2.6x10^{.3}moles of Pb^{2+} x149.1 grams of KCl }{2moles of Pb^{2+} }[/tex]
mass of KCl= 0.19383 grams
Finally, 2.6x10⁻³ moles of Pb²⁺ react with 0.19383 grams of KCl.
b) Then you can apply the following rule of three: If by stoichiometry 2 moles of Pb²⁺ produces 278.1 grams of PbCl₂, 2.6x10⁻³ moles of Pb²⁺ produces how much mass of PbCl₂?
[tex]mass of PbCl_{2} =\frac{2.6x10^{.3}moles of Pb^{2+} x278.1 grams of PbCl_{2} }{2moles of Pb^{2+} }[/tex]
mass of PbCl₂= 0.36153 grams
Finally, 2.6x10⁻³ moles of Pb²⁺ produces 0.36153 grams of PbCl₂.
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