A compound having a mass of 0 .157 g containing carbon, hydrogen, nitrogen and oxygen on combustion produces 0.213 g CO 2 and 0.0310 g H 2 O . In another experiment, 0 .103 g of the compound produces 0.0230 g NH 3 . The empirical formula of the compound with the help of these masses is to be identified. Concept introduction: For any compound, its empirical formula represents the ratio of atoms present in it. The most popular technique for evaluating the chemical formula of a compound first involves the calculation of the masses of its component elements. The moles of each element concerning each other are calculated. These moles are changed into a ratio of the whole number, which is used for the derivation of the empirical formula of a compound.
A compound having a mass of 0 .157 g containing carbon, hydrogen, nitrogen and oxygen on combustion produces 0.213 g CO 2 and 0.0310 g H 2 O . In another experiment, 0 .103 g of the compound produces 0.0230 g NH 3 . The empirical formula of the compound with the help of these masses is to be identified. Concept introduction: For any compound, its empirical formula represents the ratio of atoms present in it. The most popular technique for evaluating the chemical formula of a compound first involves the calculation of the masses of its component elements. The moles of each element concerning each other are calculated. These moles are changed into a ratio of the whole number, which is used for the derivation of the empirical formula of a compound.
Solution Summary: The author explains how the empirical formula of a compound is determined by the calculation of the masses of its component elements.
Interpretation: A compound having a mass of 0.157g containing carbon, hydrogen, nitrogen and oxygen on combustion produces 0.213g
CO2 and 0.0310g
H2O . In another experiment, 0.103g of the compound produces 0.0230gNH3 . The empirical formula of the compound with the help of these masses is to be identified.
Concept introduction: For any compound, its empirical formula represents the ratio of atoms present in it. The most popular technique for evaluating the chemical formula of a compound first involves the calculation of the masses of its component elements.
The moles of each element concerning each other are calculated. These moles are changed into a ratio of the whole number, which is used for the derivation of the empirical formula of a compound.
Predict the major organic product(s) of the following reactions. Indicate which of the following mechanisms is in operation: SN1, SN2, E1, or E2.
(c)
(4pts)
Mechanism:
heat
(E1)
CH3OH
+
1.5pts each
_E1 _ (1pt)
Br
CH3OH
(d)
(4pts)
Mechanism:
SN1
(1pt)
(e)
(3pts)
1111 I
H
10
Ill!!
H
LDA
THF (solvent)
Mechanism: E2
(1pt)
NC
(f)
Bri!!!!!
CH3
NaCN
(3pts)
acetone
Mechanism: SN2
(1pt)
(SN1)
-OCH3
OCH3
1.5pts each
2pts for either product
1pt if incorrect
stereochemistry
H
Br
(g)
“,、
(3pts)
H
CH3OH
+21
Mechanism:
SN2
(1pt)
H
CH3
2pts
1pt if incorrect
stereochemistry
H
2pts
1pt if incorrect
stereochemistry
A mixture of butyl acrylate and 4'-chloropropiophenone has been taken for proton NMR analysis. Based on this proton NMR, determine the relative percentage of each compound in the mixture
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Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY