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Inessa [10]
2 years ago
10

A reaction was set up to convert an alcohol to a carbonyl Samples of the reaction mixture were checked by infrared spectrometry

every couple of minutes. Use the infrared spectra provided to determine if the reaction mixture contains: pure alcohol, a mixture of alcohol and carbonyl, or pure carbonyl pure alcohol O pure carbonyl O mixture of alcohol and carbonyl 1000 500 O O O pure alcohol pure carbonyl mixture of alcohol and carbonyl 70

Chemistry
1 answer:
QveST [7]2 years ago
6 0

Answer:

look at peaks:

sharp peak at ~ 1700 = carbonyl

broad peak at ~ 3300 = alcohol

both = mixture

Explanation:

In the first spectrum, the broad peak occurring in the range of 3300-3700 cm-1 corresponds to OH bond stretch frequency. Carbonyl C=O bond stretch has a frequency range of 1670-1820 cm-1. The absence of any peaks in this region in the given spectrum rules out the presence of carbonyl compound in the reaction mixture. So, the reaction mixture contains only pure alcohol.

The second spectrum shows a peak around 1700 cm-1 corresponding to the carbonyl compound along with the broad peak around 3300 cm-1 corresponding to alcohol. So, the reaction mixture contains both alcohol and carbonyl compounds.

A table containing different functional groups and their corresponding Infra Red frequencies is given below for further references

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What is the volume in milliliter of 7.44 g of acetone
Mademuasel [1]

The correct answer is 9.4897 mL

It is necessary to understand a substance's mass, volume, and density in order to answer this question. By dividing a material's mass by volume, the density of the substance may be calculated. The equation for density may now be written in mathematical form using the expression for density, and the equation for mass can be produced by rearrangement using the equation for density as a starting point.

Mass of acetone = 7.44 g (given)

Volume of acetone (v) =  mass of acetone ÷ density of acetone

V = 7.44 g ÷ 0.784 g/mL

V = 9.4897 mL

Hence volume of acetone = 9.4897 mL

To learn more about density refer the link:

brainly.com/question/6107689

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7 0
1 year ago
1) An aerosol can contains gases under a pressure of 4.50 atm at 20.0 degrees Celsius. If the can is left on a hot, sandy beach,
Alika [10]

Answer:

Explanation:

1) An aerosol can contains gases under a pressure of 4.50 atm at 20.0 degrees Celsius. If the can is left on a hot, sandy beach, the pressure of the gases increases to 4.78 atm. What is the Celsius temperature on the beach?

Given data:

Initial pressure = 4.50 atm

Initial temperature = 20.0°C (20 +273 = 293 K)

Final pressure = 4.78 atm

Final temperature = ?  (in °C)

Solution:

According to the Gay-Lussac law,

The temperature of given constant amount of a gas at constant volume is directly proportional to its absolute temperature.

Mathematical expression:

P₁/T₁ = P₂/T₂

P₁ = Initial pressure

T₁ = Initial temperature

P₂ = Final pressure

T₂ = Final temperature

Now we will put the values:

P₁/T₁ = P₂/T₂

4.50 atm / 293 k = 4.78 atm / T₂

T₂ = 4.78 atm. 293 k / 4.50 atm

T₂ = 1400.54  atm.K  / 4.50 atm

T₂ = = 311.23 k

K to °C

311.23 k - 273.15 = 38.08°C

2) A sample of gas contains NO, NO2, and N2O. The pressure of the gas mixture is 4.68 atm. The pressure of NO is 501.6 mm Hg, whereas the pressure of NO2 is 2.54 atm. What is the pressure of N2O? HINT: All pressure units must be the same.

Given data:

Total pressure of gaseous mixture = 4.68 atm

Pressure of NO = 501.6 mmHg

Pressure of NO₂ = 2.54 atm

Pressure of N₂O = ?

Solution:

The given problem will be solve through the Dalton law of partial pressure.

According to this law,

" The total pressure of mixture of a gas is equal to the sum of partial pressure of all the component of gas"

Now we will convert the pressure of NO₂  in to atm.

Pressure of NO = 501.6/760 = 0.66 atm

Formula:

Total pressure = partial pressure of NO +  partial pressure of NO₂  +  partial pressure of N₂O

4.68 atm = 0.66 atm +  2.54 atm +  partial pressure of N₂O

4.68 atm = 3.2 atm +  partial pressure of N₂O

Partial pressure of N₂O = 4.68 atm - 3.2 atm

Partial pressure of N₂O = 1.48 atm

To confirm the answer:

Total pressure = partial pressure of NO +  partial pressure of NO₂  +  partial pressure of N₂O

4.68 atm =  0.66 atm +  2.54 atm +  1.48 atm

4.68 atm = 4.68 atm

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