In a 100 g sample of the compound, there are 63.57 g of carbon, 6 g of hydrogen, 9.267 g of nitrogen, and 21.17 g of oxygen. First, convert these masses into moles (n) using the formula n = m/M, where M is the molar mass from the periodic table.
For carbon: 63.57 g C -> 63.57 g C / 12.01 g/mol = 5.29 moles C.
For hydrogen: 6 g H -> 6 g H / 1.008 g/mol = 5.95 moles H.
For nitrogen: 9.267 g N -> 9.267 g N / 14.01 g/mol = 0.6615 moles N.
For oxygen: 21.17 g O -> 21.17 g O / 16.00 g/mol = 1.32 moles O.
Thus, the mole ratio looks like this: C 5.29 H 5.95 N 0.6615 O 1.32.
Now, divide each value by the smallest number (1.32): C 4 H 4.5 N 0.5 O 1.
To eliminate fractions, multiply all values by 2, yielding C8H9N1O2.
Now, all numbers are integers! Hence, the empirical formula is C8H9NO2.
Although the empirical formula isn't always the same as the molecular formula, in this instance, it corresponds to acetaminophen.
The production mechanism for t-butyl alcohol proceeds as follows:
The reaction and corresponding rate law for isobutene adsorption on the Amberlyst-15 catalyst can be described by:
I + S ⇄ I * S 
where 
represents the concentration of unoccupied sites
denotes the adsorption equilibrium constant
indicates the forward rate constant
are the concentrations of isobutene and the site occupied by isobutene
The equation for the adsorption of water (W) onto the Amberlyst-15 catalyst is outlined as:
W + S ⇄ W.S 
The surface reaction's rate law can be described as:
W.S + I.S ⇄ TBA. S + Sn 
The desorption rate law for TBA from the catalyst is as follows:
TBA. S ⇄ TBA + S 
The image included below illustrates the rest of the steps.
a) The completely balanced chemical reaction is:
Zn(s) + H2SO4(aq)
--------> ZnSO4(aq) + H2 (g)
<span>b) Initially, we determine the quantity of zinc that has reacted based on the produced H2.</span>
According to stoichiometry, 1 mole of Zn is required for each mole of H2 created, thus:
moles(Zn) = moles(H2)
where moles are calculated as the ratio of mass to molar mass (MM)
mass(Zn) / MM(Zn) = mass(H2) / MM(H2)
mass(Zn) = [mass(H2) / MM(H2)] * MM(Zn)
mass(Zn) = [(0.0764 g)/(2 g/mol)] * 65.38 g/mol
mass(Zn) = 2.49 g
Consequently, we find 2.49 g of pure zinc in the sample, leading to a purity of zinc of:
purity = (2.49 / 3.86) * 100 % = 64.50 %
<span>c) In part (b), it is assumed that the impurities in the sample do not react with sulfuric acid to emit hydrogen.
Thus, the hydrogen solely arises from the reaction of Zn with sulfuric acid.</span>
