Respuesta :
Mg²⁺ + 2Cl⁻ = MgCl₂
n(Mg²⁺)=0.25 mol
n(Cl⁻)=2n(Mg²⁺)
n(Cl⁻)=2*0.25=0.50 mol
n(Mg²⁺)=0.25 mol
n(Cl⁻)=2n(Mg²⁺)
n(Cl⁻)=2*0.25=0.50 mol
Answer:
0.50 moles of Cl-
Explanation:
Magnesium is an alkaline earth metal and belongs to group II A in the periodic table. The oxidation state of Mg is +2 i.e. it forms a doubly charged cation Mg2+
Chloride is a halogen and belongs to group VII A in the periodic table. The oxidation state is -1 i.e. it forms an anion, Cl-
When Mg2+ and Cl- combine, the product formed is an ionic compound MgCl2. The balanced equation is:
Mg^{2+}+ 2Cl^{-}\rightarrow MgCl_{2}
2 moles of Cl- ions combine with 1 mole of Mg2+ to form the product
i.e. the ratio of Mg2+ : Cl- = 1:2
Therefore, 0.25 moles of Mg2+ would need 0.50 moles of Cl-
