Respuesta :
Answer: The mass of chlorine produced in the given reaction is 13.206 grams.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] Â Â Â .....(1)
- For manganese oxide:
Given mass of manganese oxide = 16.0 g
Molar mass of manganese oxide = 86.9 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of manganese oxide}=\frac{16g}{86.9g/mol}=0.184mol[/tex]
- For hydrochloric acid:
Given mass of hydrochloric acid = 30.0 g
Molar mass of hydrochloric acid = 36.5 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of hydrochloric acid}=\frac{30g}{36.5g/mol}=0.822mol[/tex]
For the given chemical reaction:
[tex]MnO_2+4HCl\rightarrow MnCl_2+Cl_2+2H_2O[/tex]
By Stoichiometry of the reaction:
1 mole of manganese oxide reacts with 3 moles of hydrochloric acid.
So, 0.184 moles of manganese oxide will react with = [tex]\frac{3}{1}\times 0.184=0.736moles[/tex] of hydrochloric acid
As, given amount of hydrochloric acid is more than the required amount. So, it is considered as an excess reagent.
Thus, manganese oxide is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of manganese oxide reacts with 1 moles of chlorine.
So, 0.184 moles of manganese oxide will react with = [tex]\frac{1}{1}\times 0.184=0.184moles[/tex] of chlorine.
Now, calculating the mass of chlorine from equation 1, we get:
Molar mass of chlorine = 71 g/mol
Moles of chlorine = 0.186 moles
Putting values in equation 1, we get:
[tex]0.186mol=\frac{\text{Mass of chlorine}}{71g/mol}\\\\\text{Mass of chlorine}=13.206[/tex]
Hence, the mass of chlorine produced in the given reaction is 13.206 grams.
