# Answer to Question #56086 in General Chemistry for jocelyn

Question #56086

NaCl-58.4 g/mol - 60.7%Cl

MgCl2- 95.2g.mol - 74.5% Cl

Fecl3- 162.2g/mol - 65.6% Cl

assume that you had 0.00g of each chloride compound

A) how many moles of each compound would this represent in each case

B) how many moles of Cl would be present in each case

C) how many moles of AgCl would you expect to recover from the precipitation reaction in each case?

D) what mass of AgCl (MW=143.3g/mol) would this represent for each case

MgCl2- 95.2g.mol - 74.5% Cl

Fecl3- 162.2g/mol - 65.6% Cl

assume that you had 0.00g of each chloride compound

A) how many moles of each compound would this represent in each case

B) how many moles of Cl would be present in each case

C) how many moles of AgCl would you expect to recover from the precipitation reaction in each case?

D) what mass of AgCl (MW=143.3g/mol) would this represent for each case

Expert's answer

A) If we have 0.00g – we have 0.00 moles of each compound

B) If we have 0.00g - 0.00 moles of Cl

C) If we have 0.00g – 0.00 moles of AgCl

D) 0.00 g of AgCl

B) If we have 0.00g - 0.00 moles of Cl

C) If we have 0.00g – 0.00 moles of AgCl

D) 0.00 g of AgCl

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