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Gekata [30.6K]
2 years ago
10

Does the ir spectrum allow you to confirm that the structure of the product is a combination of the two reactants?

Chemistry
1 answer:
krok68 [10]2 years ago
5 0

Yes, the IR spectrum allow you to confirm that the structure of the product is a combination of the two reactants.

<h3>What is Spectrum?</h3>
  • A spectrum is a state that can fluctuate without gaps across a continuum and is not constrained to a particular range of values.
  • After passing through a prism, visible light takes on a rainbow of hues, which is how the term was initially used scientifically in optics.
  • As knowledge of light increased on a scientific level, it started to encompass the full electromagnetic spectrum.
  • As a result, it evolved into a mapping of a variety of magnitudes to a variety of qualities, including the perceived "colours of the rainbow" and other attributes that correspond to wavelengths outside of the spectrum.
  • Today, analogies with spectrum are used to discuss subjects unrelated to optics.

Learn more about spectrum here:

brainly.com/question/14282264

#SPJ4

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In the previous problem, which are the limiting reactants for each reaction? Based on this, calculate the maximum yield of oxyge
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please show the previous problem


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3 years ago
Within a period, the nuclear charge increases as you move from left to right across the
a_sh-v [17]

Answer:

The answer is Ionization energy.

Explanation:

Ionization Energy. The ionization energy tends to increase as one moves from left to right across a given period or up a group in the periodic table.

3 0
3 years ago
Analysis of a gaseous chlorofluorocarbon, CClxFy, shows that it contains 11.79% C and 69.57% Cl. In another experiment, you find
uranmaximum [27]

Answer:

The molecular formula = C_2Cl_{4}F_2

Explanation:

Moles =\frac {Given\ mass}{Molar\ mass}

% of C = 11.79

Molar mass of C = 12.0107 g/mol

<u>% moles of C = 11.79 / 12.0107 = 0.9816</u>

% of Cl = 69.57

Molar mass of Cl = 35.453 g/mol

<u>% moles of Cl = 69.57 / 35.453 = 1.9623</u>

Given that the gaseous chlorofluorocarbon only contains chlorine, flourine and carbon. So,

% of F = 100% - % of C - % of C = 100 - 11.79 - 69.57 = 18.64

Molar mass of F = 18.998 g/mol

<u>% moles of F = 18.64 / 18.998 = 0.9812</u>

Taking the simplest ratio for C, Cl and F as:

0.9816 : 1.9623 : 0.9812

= 1 : 2 : 1

The empirical formula is = CCl_2F

Also, Given that:

Pressure = 21.3 mm Hg

Also, P (mm Hg) = P (atm) / 760

Pressure = 21.3 / 760 = 0.02803 atm

Temperature = 25 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (25 + 273.15) K = 298.15 K  

Volume = 458 mL  = 0.458 L (1 mL = 0.001 L)

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.02803 atm × 0.458 L = n × 0.0821 L.atm/K.mol × 298.15 K  

⇒n = 0.00052445 moles

Given that :  

Amount  = 0.107 g  

Molar mass = ?

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.00052445= \frac{0.107\ g}{Molar\ mass}

Molar\ mass= 204.0233\ g/mol

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 1×12.0107 + 2×35.453 + 1×18.998 = 101.9147 g/mol

Molar mass = 204.0233 g/mol

So,  

Molecular mass = n × Empirical mass

204.0233 = n × 101.9147

⇒ n = 2

<u>The molecular formula = C_2Cl_{4}F_2</u>

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3 years ago
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1.5 liters are in 1,500cm^3.
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3 years ago
Uranium-235 and uranium-238 are considered isotopes of one another
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If you are asking which is the most abundant, Uranium-238 is
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