A 1.0000 gram sample of zinc metal is added to a solution containing 1.2500 gram

Question

A 1.0000 gram sample of zinc metal is added to a solution containing 1.2500 grams of an unknown compound made of bismuth and chlorine. The reaction results in teh formation of zinc chloride and metallic bismuth. when the reaction is complete, unreacted zinc remains, and this unreacted zinc is "burned off" by reaction with hydrochloric acid. After washing and drying, the mass of bismuth metal recovered is 0.6763 grams.

1) Calculate thh experimental percentage of bismuth in the original unknown compound.

2) if 2.300 g of the unknown bismuth chloride has been used, how many grams of chlorine would you expect it to contain.?

3) determine the empirical formula of the original unknown compound.

4) Write a balanced chemical equation for the reaction of zinc with the original unknown compound.

5) assuming that your answer to part 4 is correct, what is the minimum mass of zinc metal needed to react with the original bismuth chloride compound.?

Explanation / Answer

d) the zinc must react to produce the zinc chloride and zinc fluoride, The Nb does not react

Equation: 2NbCl3F2 + 5Zn = 2Nb + 3ZnCl2 + 2ZnF2

e) Determine the mass of Zn required to react with 1.2500g NbCl3F2
From the equation:
2mol NbCl3F2 will react with 5mol Zn

Molar mass NbCl3F2 = 237.2628 g/mol
1.2500g NbCl3F2 = 1.2500/237.2628 = 0.005268mol
This will react with : 0.005268 *5/2 = 0.0132 mol Zn
Molar mass Zn = 65.38g/mol
0.0132mol = 0.0132 * 65.38 = 0.86g

Mass Zn required = 0.86g.

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