This reaction forms triphenylmethanol from benzophenone. How could you use infrared spectroscopy to show that the benzophenone h
ad reacted (been consumed) and that the product of the reaction was triphenylmethanol
1 answer:
Complete Question
The complete question is shown on the first uploaded image
Answer:
The consumption of the reactant benzophenone and the production of triphenylmethanol can be detected using their IR absorption spectrum
This reaction is shown on the second uploaded image
The reactant benzophenone is a compound which contains a carbonyl functional group, and the stretching frequency of C=O bond has a high absorption at around and frequency band of this wavelength is absent in triphenylmethanol.
in the same vain the product triphenylmethanol is a compound which contains a hydroxyl (OH) functional group, and the stretching frequency of O-H bond has a high absorption at around and frequency band of this wavelength is absent in benzophenone.
To use infrared spectroscopy to show that the reaction is occurring is to show the disappearance of the frequency band which indictes the consumption of benzophenone and the appearance
frequency band which indictes the formation of triphenylmethanol
Explanation:
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14.292 grams of Fe2O3 is formed when 10 gram of iron metal is burned.
Explanation:
The balanced equation for the reaction is to be known so that number of moles taking part can be known.
The balanced chemical equation is
4Fe + 3⇒ 2
From the given weight of iron to be used for the production of , number of moles of Fe taking part in the reaction can be known by the formula:
Number of moles= mass ÷ Atomic mass of one mole of the element.
(Atomic weight of Fe is 55.845 gm/mole)
Putting the values in equation
Number of moles = 10 gm ÷ 55.845 gm/mole
= 0.179 moles
Applying the stoichiometry concept
4 moles of Fe gives 2 Moles of Fe2O3
0.179 moles will produce x moles of Fe2O3
So, 2÷ 4 = x ÷ 0.179
2/4 = x/ 0.179
2 × 0.179 = 4x
2 × 0.179 / 4 = x
x = 0.0895 moles
So from 10 grams of iron metal 0.0895 moles of Fe2O3 is formed.
Now the formula used above will give the weight of Fe2O3
weight = atomic weight × number of moles
= 159.69 grams × 0.0895
= 14.292 grams of Fe2O3 formed.