Right now I’m a freshmen, and we got our scheduling paper for next year as sophomores. I’m wondering if I should take chemistry
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<u>Answer:</u> The mass of cryolite produced is 51.48 kg
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For aluminium oxide:</u>
Given mass of aluminium oxide = 12.5 kg = 12500 g (Conversion factor: 1 kg = 1000 g)
Molar mass of aluminium oxide = 101.96 g/mol
Putting values in equation 1, we get:
- <u>For NaOH:</u>
Given mass of NaOH = 55.4 kg = 55400 g
Molar mass of NaOH = 40 g/mol
Putting values in equation 1, we get:
- <u>For HF:</u>
Given mass of HF = 55.4 kg = 55400 g
Molar mass of HF = 20 g/mol
Putting values in equation 1, we get:
For the given chemical reaction:
By Stoichiometry of the reaction:
1 mole of aluminium oxide reacts with 6 moles of sodium hydroxide and 12 moles of HF.
So, 122.6 moles of aluminium oxide will react with of sodium hydroxide and
of HF
As, given amount of NaOH and HF is more than the required amount. So, they are considered as an excess reagent.
Thus, aluminium oxide is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of aluminium oxide produces 2 moles of cryolite
So, 122.6 moles of aluminium oxide will produce = of cryolite
Now, calculating the mass of cryolite by using equation 1:
Molar mass of cryolite = 209.94 g/mol
Moles of cryolite = 245.2 mol
Putting values in equation 1, we get:
Converting this into kilograms, we use the conversion factor:
1 kg = 1000 g
So,
Hence, the mass of cryolite produced is 51.48 kg