How much mass (in grams) is in a 3.25 mol sample of NH4OH?
1 answer:
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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: