If a given solution has a 30 percent solute concentration, and more solute is added to the solution, the new solute concentratio
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<u>Answer:</u> The mass of aluminium chloride that can be formed are 46.3 g
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
....(1)
- <u>For Aluminium:</u>
Given mass of aluminium = 32 g
Molar mass of aluminium = 26.98 g/mol
Putting values in above equation, we get:
- <u>For Chlorine:</u>
Given mass of chlorine = 37 g
Molar mass of chlorine = 71 g/mol
Putting values in above equation, we get:
For the given chemical equation:
By Stoichiometry of the reaction:
3 moles of chlorine gas is reacting with 2 moles of aluminium.
So, 0.521 moles of chlorine gas will react with = of aluminium.
As, given amount of aluminium is more than the required amount. Thus, it is considered as an excess reagent.
So, chlorine gas is considered as a limiting reagent because it limits the formation of products.
By Stoichiometry of the reaction:
3 moles of chlorine gas is producing 2 moles of aluminium chloride
So, 0.521 moles of chlorine gas will react with = of aluminium chloride.
Now, calculating the mass of aluminium chloride by using equation 1, we get:
Moles of aluminium chloride = 0.347 moles
Molar mass of aluminium chloride = 133.34 g/mol
Putting all the values in equation 1, we get:
Hence, the mass of aluminium chloride that can be formed are 46.3 g
Answer: False.
The final pressure in the system is 4.14 atm
Explanation: Please see the attachments below
