What would be the pressure of a 5.00 mol sample of Cl₂ at 400.0 K in a 2.00 L container found using the van der Waals equation?
1 answer:
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Explanation:
Using Beer-Lambert's law :
Formula used :
where,
A = absorbance of solution
c = concentration of solution
l = length of the cell
= molar absorptivity of this solution
According to question:
A = (C) : absorbance measured by the spectrometer
c = (B) : concentration, in mol/L, of the stock solution from which the sample was made
l = (A): pathlength of light through the cell
ε = (D) : molar absorptivity, a constant unique to that substance at that wavelength
Answer:
0.2042 M is the original concentration of (aq) in the titrating solution.
Explanation:
Mass of = 0.217 g
Moles of
1 mole of have 2 mole of As and 1 mole of
have 1 mole of As.
So, from 1 mole of we will have 2 moles of
Then from 0.001096 mol of :
of
According to reaction, 1 mole of reacts with 2 mole of cerium (IV) ions,then 0.002192 mol of
of cerium (IV) ions.
Volume of the acidic cerium{IV) sulfate = 21.47 ml =0.02147 L
1 mL = 0.001 L
0.2042 M is the original concentration of (aq) in the titrating solution.