An unknown compound a has the molecular formula c7h14o2. compound a absorbs strongly in the ir at 1700 cm-1. the 1h nmr spectral
data for compound a are given below. what is the structure of compound a?
2 answers:
The structure of compound a is as shown in the figure a
<h3>Further explanation</h3>A chemical compound is the chemical substance composed of many identical molecules and it composed of atoms from more than one element held together by chemical bonds. Ethyl isovalerate or is an organic compound that is the ester formed from ethyl alcohol and isovaleric acid. It has a fruity odor and flavor and useful for perfumery and food additive.
Nuclear magnetic resonance spectroscopy, most commonly known as NMR spectroscopy is the analytical chemistry technique for quality control and reserach to determine the content and purity of a sample as well as its molecular structure. NMR can quantitatively analyze mixtures containing known compounds.
An unknown compound a has the molecular formula . Compound a absorbs strongly in the IR at
. the 1h NMR spectral data for compound a are given below. what is the structure of compound a?
The structure of compound a is as shown in the figure a, because the structure of compound a would be solid and dense enough for antimicrobial form
<h3>Learn more</h3>- Learn more about compound brainly.com/question/1775854
- Learn more about molecular formula brainly.com/question/8316933
- Learn more about nmr brainly.com/question/10206242
Grade: 9
Subject: chemistry
Chapter: nmr
Keywords: compound, molecular formula, c7h14o2, ir, nmr
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If you place 1.0 L of ethanol (C2H5OH) in a small laboratory that is 3.0 m long, 2.0 m wide, and 2.0 m high, will all the alcohol evaporate? If some liquid remains, how much will there be? The vapor pressure of ethyl alcohol at 25 °C is 59 mm Hg, and the density of the liquid at this temperature is 0.785g/cm^3 .
will all the alcohol evaporate? or none at all?
Answer:
Yes, all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore be zero.
Explanation:
Given that:
The volume of alcohol which is placed in a small laboratory = 1.0 L
Vapor pressure of ethyl alcohol at 25 ° C = 59 mmHg
Converting 59 mmHg to atm ; since 1 atm = 760 mmHg;
Then, we have:
=
= 0.078 atm
Temperature = 25 ° C
= ( 25 + 273 K)
= 298 K.
Density of the ethanol = 0.785 g/cm³
The volume of laboratory = l × b × h
= 3.0 m × 2.0 m × 2.5 m
= 15 m³
Converting the volume of laboratory to liter;
since 1 m³ = 100 L; Then, we have:
15 × 1000 = 15,000 L
Using ideal gas equation to determine the moles of ethanol in vapor phase; we have:
PV = nRT
Making n the subject of the formula; we have:
n = 47. 88 mol of ethanol
Moles of ethanol in 1.0 L bottle can be calculated as follows:
Since numbers of moles =
and mass = density × vollume
Then; we can say ;
number of moles =
number of moles =
number of moles =
number of moles = 17.039 mol
Thus , all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore be zero.