Hi does anyone have the data table answers for the Charles Law Lab Report from Edge?
1 answer:
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Answer:
a) 35.485 moles of Al(SO)
b) 35.485 moles of S atoms
c) Al atoms
d) 567.723 g of O
Explanation:
Let's define the following terms :
1 mol = elemental units
For example :
1 mol of oxygen atoms = oxygen atoms
Now, our compound has the following formula
Al(SO)
Where Al is aluminium
S is sulfur
And O is oxygen
All the subscripts are 1 so we can say the following :
1 molecule of Al(SO) has 1 atom of Al , 1 atom of S and 1 atom of O
In terms of moles :
1 mol of Al(SO) has 1 mol of Al , 1 mol of S and 1 mol of O
The molar masses of Al, S and O are
If we sum all the molar masses =
Finally, 75.046 g of Al(S0) is 1 mol of Al(SO) which contains 26.982 g of Al, 32.065 g of S and 15.999 g of O.
1 mol of Al(SO) contains 1 mol of Al, 1 mol of S and 1 mol of O.
Now we can calculate a),b),c) and d)
For a)
75.046 g of Al(SO) = 1 mol of Al(SO)
2663 g of Al(SO) = x
2.663 kg of Al(SO) contains 35.485 moles of Al(SO)
b) and c) 1 mol of Al(SO) molecules contains 1 mol of S atoms and 1 mol of Al atoms
We have 35.485 moles of Al(SO) molecules so
We have 35.485 moles of S atoms
And 35.485 moles of Al atoms
If 1 mol =
35.485 moles of Al have Al atoms
d) 75.046 g of Al(SO) contains 15.999 g of O
2663 g of Al(SO) contains x g of O
x = 567.723 g of O
Answer:
4.1x10⁻⁵
Explanation:
The dissociation of an acid is a reversible reaction, and, because of that, it has an equilibrium constant, Ka. For a generic acid (HA), the dissociation happens by:
HA ⇄ H⁺ + A⁻
So, if x moles of the acid dissociates, x moles of H⁺ and x moles of A⁻ is formed. the percent of dissociation of the acid is:
% = (dissociated/total)*100%
4.4% = (x/[HA])*100%
But x = [A⁻], so:
[A⁻]/[HA] = 0.044
The pH of the acid can be calcualted by the Handersson-Halsebach equation:
pH = pKa + log[A⁻]/[HA]
3.03 = pKa + log 0.044
pKa = 3.03 - log 0.044
pKa = 4.39
pKa = -logKa
logKa = -pKa
Ka =
Ka =
Ka = 4.1x10⁻⁵