Question

Problem 6.144

A 2.197 g sample of an unknown alkaline-earth metal was allowed to react with a volume of chlorine gas that contains 1.91×1022Cl2 molecules. The resulting metal chloride was analyzed for chlorine by dissolving a 0.623 g sample in water and adding an excess of AgNO3(aq) to give a precipitate of 1.126 g of solid AgCl.

A

What is the percent Cl in the alkaline-earth chloride? = 44.7%

What is the identity of the alkaline-earth metal? = Sr

*Write balanced equation for first chemical reaction.

Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

A:- First reaction:-

Sr (s)     + Cl₂ (g)     ------------->     SrCl₂ (s)    

Second reaction:-

SrCl₂ (s)    +   2 AgNO₃ (aq)   -------->    2 AgCl (s)    +    Sr(NO₃)₂ (aq)