A student followed a procedure to determine the empirical formula of a compound

Question

A student followed a procedure to determine the empirical formula of a compound of inron (Fe) and Cl. She added a 2,15g piece of Zn to a solution containing 1.750g of FeCl. After the reation was complete .771 g of Fe was isolated.

a. calculate the mass of Cl in the solution

b. calculate the number of moles of Fe present

c. calculate the number of moles of Cl present

d. Determine the molar ratio of Fe to Cl in the compound. Use this ratio to write the empirical formule of the compunt of iron and chloribe.

PLEASE SHOW ALL WORK AND CALCULATIONS

Explanation / Answer

Our compound is FexCly x and y are numbers that will complete the empirical formula.

Zn + FexCly -----> Fe + ZnCl2

a) mass Cl= mass FexCly - mass Fe= 1.75g - 0.771g= 0.979g

b) mol Fe present= 0.771g/56g/mol= 0.014 mol

c) mol Cl= 0.979g/35.45g/mol= 0.028 mol

d) molar ratio Cl: 0.028/0.014= 2

molar ratio Fe: 0.014/0.014= 1

empirical formula: FeCl2

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