Elements in group 1 will (lose or gain) electrons to obtain a noble gas structure. How many electrons will the element gain or l
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Answer : The percent purity of in the original sample is 87.94 %
Explanation :
The given balanced chemical reaction is:
First we have to calculate the mass of Fe.
Molar mass of Fe = 55.8 g/mole
Now we have to calculate the moles of
From the balanced chemical reaction we conclude that,
As, 2 moles of Fe produced from 1 mole of
So, of Fe produced from
mole of
Now we have to calculate the mass of
Molar mass of = 159.69 g/mole
Now we have to calculate the percent purity of in the original sample.
Mass of original sample =
Therefore, the percent purity of in the original sample is 87.94 %
Taking into account the reaction stoichiometry, 1.119 grams of chlorine gas are required to produce 3.32 grams of bismuth chloride is produced.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
2 Bi + 3 Cl₂ → 2 BiCl₃
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- Bi: 2 moles
- Cl₂: 3 moles
- BiCl₃: 2 moles
The molar mass of the compounds is:
- Bi: 209 g/mole
- Cl₂: 70.90 g/mole
- BiCl₃: 315.45 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
Bi: 2 moles ×209 g/mole=418 g
Cl₂: 3 moles ×70.90 g/mole= 212.7 g
BiCl₃: 2 moles ×315.45 g/mole= 630.9 g
<h3>Mass of Cl₂ required</h3>The following rule of three can be applied: If by reaction stoichiometry 630.9 grams of BiCl₃ are formed by 212.7 grams of Cl₂, 3.32 grams of BiCl₃ are formed by how much mass of Cl₂?
<u><em>mass of Cl₂= 1.119 grams</em></u>
Finally, 1.119 grams of chlorine gas are required to produce 3.32 grams of bismuth chloride is produced.
Learn more about the reaction stoichiometry: